10.50 kg of iron will be produced from 15 kg of iron (III) oxide.
What is mass?The amount of matter in an item is measured by its mass, which is a fundamental physical quantity. It is a scalar amount that is measured in kilograms (kg) or grams (g). Regardless of an object's location or the force pressing against it, its mass always remains constant.
How do you determine it?Iron (III) oxide and elemental iron react chemically in the following balanced chemical equation:
2 Fe2O3+ 3 C = 4 Fe + 3 CO2
Due to the reaction between 2 moles of Fe2O3 and 4 moles of Fe, the mole ratio of Fe2O3 to Fe is either 2:4 or 1:2.
The amount of iron created from 15 kg of Fe2O3 can be calculated using this mole ratio:
Fe2O3 = 2 moles of Fe per mole.
Fe2O3's molecular weight is 159.69 g/mol.
Fe2O3 has a mass of 15 kg and a density of 15,000 g/mol, or 94.00 moles.
We can figure out how many moles of Fe were produced using the mole ratio of 1:2:
We can figure out how many moles of Fe were produced using the mole ratio of 1:2:
2 moles of Fe for each mole of Fe2O3 94.00 moles of Fe2O3 multiplied by (2 moles of Fe for each mole of Fe2O3) results in 188.00 moles of Fe.
The molar mass of Fe can then be used to convert the moles of iron to mass as follows:
Fe's molecular weight is 55.85 g/mol.
188.00 moles of Fe produced at a rate of 55.85 g/mol result in a mass of 10,499.80 g or 10.50 kg.
Hence, 10.50 kg of iron will be produced from 15 kg of iron (III) oxide.
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3) The following reaction is at equilibrium, when pressure is increased:
H₂(g) + CO2(g) + heat H₂O(g) + CO(g)
10
A. In order to restore equilibrium, the reaction shifts left, toward reactants
B. In order to restore equilibrium, the reaction shifts right, toward products
C. No change occurs
The effect of increasing pressure on the given equilibrium reaction:
H₂(g) + CO₂(g) + heat ⇌ H₂O(g) + CO(g)
is determined by the stoichiometry of the reaction and the number of moles of gas on each side of the equation.
On the left-hand side, there are two moles of gas (H₂ and CO₂), whereas on the right-hand side, there are only one mole of gas (CO). Therefore, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, in order to decrease the overall pressure.
In this case, the reaction will shift towards the right, towards the products, to decrease the pressure. Therefore, the correct answer is:
B. In order to restore equilibrium, the reaction shifts right, toward products.
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How many carbon atoms are in 11.5 g C2H5OH?
There are approximately 3.02 x 10²³ carbon atoms in 11.5 g of [tex]C_{2}H_{5} OH[/tex]
To calculate the number of carbon atoms present in the 11.5g of [tex]C_{2}H_{5}OH[/tex]which is ethanol, we need to find and calculate the number of moles of ethanol present and convert moles to the number of carbon atoms by using Avogadro's number.
The molecular weight of [tex]C_{2}H_{5}OH[/tex] is =
no. of atoms x its atomic weight. So the molecular weight is,
(2 atoms of carbon x 12 g/mol )+ (5 atoms of hydrogen x 1 g/mol) + (1 atom of oxygen x 16 g/mol) + (1 atom of hydrogen x 1 g/mol ) =
24+10+16+1 ≅ 47 g/mol
The number of moles of ethanol = given mass / molecular weight = 11.5g /47 g/mol = 0.2446 moles
Number of Carbon atoms = no. of moles of ethanol x Avogadro number x no. of carbon atoms in each molecule of ethanol = 0.2446 moles x 6.022 x 10²³ atoms/mol x 2 carbon atoms/molecule ≅ 3.02 x 10²³
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Compare and contrast the four different types of solar activity above the photosphere. (Select all that apply)
A. Prominences are huge loops of the Sun’s ionized but cool material that are pushed by magnetic forces from the chromosphere into the corona.
B. There are regions of higher density and temperature than the surrounding material in the chromosphere called plages.
C. Flares are long lived phenomena above the photosphere beginning at the solar minimum and ending at solar maximum.
D. Coronal mass ejections happen when a flare is so violent that the material exceeds the escape speed of the sun. It is connected to sunspots.
There are up to four different kinds of features that can be seen when viewing the photosphere. Sunspots, faculae, granulation, and super-granulation are listed in decreasing order of observational ease. All the given statement are true.
Solar activityIn the chromosphere, plateaus are areas that are more dense and hotter than the surrounding material. Large, chilly, ionized loops of material known as prominences are slowly pushed into the corona by magnetic energy from the chromosphere. Flares are erratic, fiery, and intensely energetic bursts that last only a moment or two. When a flare is extremely powerful, its material is thrown into the solar system beyond the Sun's escape velocity and causes coronal mass ejections. These are all essentially connected to sunspots.For more information on solar activity above photosphere kindly visit to
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A compound has a similar molecular mass of 180grams/mol. It contains 40.8% carbon,5.8% hydrogen and 53.4% oxygen. Calculate its empirical formula and molecular formula, and give its common name.
Answer:
To find the empirical formula of the compound, we need to determine the simplest whole-number ratio of atoms in the molecule.
First, we can assume that we have 100 grams of the compound, and calculate the number of moles of each element present in it:
Carbon: 40.8 g / 12.011 g/mol = 3.398 mol
Hydrogen: 5.8 g / 1.008 g/mol = 5.753 mol
Oxygen: 53.4 g / 15.999 g/mol = 3.337 mol
Next, we divide each of these values by the smallest one, which is 3.337, to get the mole ratio:
Carbon: 3.398 mol / 3.337 mol = 1.019
Hydrogen: 5.753 mol / 3.337 mol = 1.723
Oxygen: 3.337 mol / 3.337 mol = 1.000
Rounding these values to the nearest whole number, we get the empirical formula: C1.0H1.7O1.0, which can be simplified to CH1.7O.
To find the molecular formula, we need to know the actual molecular mass of the compound. We can estimate it by adding the atomic masses of the elements in the empirical formula:
Carbon: 1 x 12.011 = 12.011
Hydrogen: 1.7 x 1.008 = 1.714
Oxygen: 1 x 15.999 = 15.999
Total = 29.724 g/mol (approx.)
The molecular mass is close to 180 g/mol, which suggests that the actual molecular formula is a multiple of the empirical formula. Dividing 180 by 29.724, we get a value of about 6.05. Multiplying the subscripts in the empirical formula by this value, we get the molecular formula: C6H10.2O6, which can be further simplified to C3H5.1O3.
The compound with the empirical formula CH1.7O and the molecular formula C3H5.1O3 is commonly known as glyoxylic acid.
Sucrose (C12H22011) is combusted in air according to the following reaction:
C12H22011(s) + O2(g) = CO2(g) + H2O(l )
How many moles of carbon dioxide would be produced by the complete combustion of 38.5 grams of sucrose in the presence of excess oxygen?
Okay, let's break this down step-by-step:
1) The molecular formula for sucrose is C12H22011. This means each mole of sucrose contains 12 moles of carbon and 22 moles of hydrogen.
2) You are combusting 38.5 grams of sucrose. To convert grams to moles, we divide by the molar mass:
Molar mass of C12H22011 = 342.3 g/mol
So 38.5 g / 342.3 g/mol = 0.113 moles of sucrose
3) According to the combustion reaction, each mole of sucrose produces 12 moles of CO2.
So 0.113 moles of sucrose will produce 0.113 * 12 = 1.356 moles of CO2.
4) Round to the nearest whole number:
1 mole of CO2
Therefore, the complete combustion of 38.5 grams of sucrose in excess oxygen would produce 1 mole of carbon dioxide.
Let me know if you have any other questions!
Select the correct answer. A certain reaction has this form:aA bB. At a particular temperature and [A]0 = 2.00 x 10-2 Molar, concentration versus time data were collected for this reaction and a plot of ln[A]t versus time resulted in a straight line with a slope value of -2.97 x 10-2 min-1. What is the reaction order and rate law for this reaction? A. first, rate = k[A] B. first, rate = k[A]2 C. second, rate = k[A] D. second, rate = k[A]2 E. third, rate = k[A]
The reaction order and rate law for this reaction is first, rate = k[A]. Option A is correct.
The reaction order and rate law for a reaction can be determined from the slope of a plot of ln[A] versus time.
Given that the plot of ln[A] versus time resulted in a straight line with a slope value of -2.97 x 10⁻² min⁻¹, we can determine the reaction order and rate law as follows;
If the slope is equal to 1, the reaction order is 1st order.
If the slope is equal to 2, the reaction order is 2nd order.
If the slope is equal to 3, the reaction order is 3rd order.
From the given slope of -2.97 x 10⁻² min⁻¹, we can conclude that the reaction order is 1st order, because the slope value is equal to -1 times the reaction order. So, the reaction order for this reaction is 1st order.
The rate law for a 1st order reaction will be given by;
rate = k[A]
where [A] is the concentration of the reactant, and k is the rate constant.
Therefore, first, rate = k[A].
Hence, A. is the correct option.
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Give the number of significant figures indicated.
0.066
Reaction A: consider a solution of acetophenone (AKA methyl phenyl ketone) and sodium trifluoroperacetate (deprotonated trifluoroperacetic acid). Draw these two reactants and then show a full arrow-pushing mechanism providing the flow of electrons, showing how the two react with one another and the resulting product
The concept Beckmann rearrangement is used here in order to show the reaction between acetophenone (AKA methyl phenyl ketone) and sodium trifluoroperacetate. The product formed is acetaminophen.
In simple Beckmann rearrangement is a reaction in which oxime is changed to an amide under some acidic conditions. The oxime is obtained by treating an aldehyde or a ketone with hydroxylamine.
This Beckmann rearrangement reaction is named after Ernst Otto Beckmann who is a German scientist. It is used for producing various drugs and steroids.
The mechanism of the Beckmann reaction is given below:
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Which of the following reactants lead to the fastest reaction?
A) Solid aluminum and oxygen
B) Sodium hydroxide and hydrogen chloride in water
C) Copper nitrate and ethanol in water
D) Solid barium chloride and sodium sulfate
Solid aluminum and oxygen are the reactant that lead to the fastest reaction. Therefore, the correct option is option A.
Chemical reaction, the transformation of one or more chemicals (the reactants) into one or more distinct compounds (the products). Chemical elements or chemical compounds make up substances.
Chemical reactions constitute a fundamental component of life itself, as well as technology and culture. Burning fuels, melting iron, creating glass or pottery, brewing beer, making wine. Solid aluminum and oxygen are the reactant that lead to the fastest reaction.
Therefore, the correct option is option A.
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The cell diagram for a silver‑zinc button battery is Zn(s),ZnO(s)∣∣KOH(aq)∣∣Ag2O(s),Ag(s) Write the balanced half‑reaction that occurs at the anode during discharge. anode half-reaction: Write the balanced half‑reaction that occurs at the cathode during discharge. cathode half-reaction: Write the balanced overall cell reaction that occurs during discharge. overall cell reaction:
Voltaic or galvanic (spontaneous) cells are denoted by cell notations in shorthand is cathode.
Thus, This special shorthand describes the anode, cathode, and electrode components as well as the reaction circumstances.
Recall that reduction occurs at the cathode whereas oxidation occurs at the anode. Electrons go from the anode to the cathode when the anode and cathode are connected by a wire.
First, the cathode half-cell is detailed, then the anode half-cell. The reactants are mentioned first and the products are specified last within a specific half-cell.
Thus, Voltaic or galvanic (spontaneous) cells are denoted by cell notations in shorthand is cathode.
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Calculate the molality of a solution prepared by dissolving 19.9 g of KCl in 750.0 mL of water.
Answer:
Explanation:
First, we need to calculate the moles of KCl:
Calculate the molar mass of KCl:
KCl = 39.10 g/mol (atomic weight of K) + 35.45 g/mol (atomic weight of Cl)
= 74.55 g/mol
Calculate the moles of KCl:
moles of KCl = mass of KCl / molar mass of KCl
= 19.9 g / 74.55 g/mol
= 0.267 mol
Next, we need to convert the mass of the solvent (water) from milliliters to kilograms:
Convert mL to L:
750.0 mL = 750.0 mL * (1 L / 1000 mL)
= 0.7500 L
Calculate the mass of water:
mass of water = volume of water x density of water
= 0.7500 L x 1000 g/L
= 750.0 g
Convert the mass of water to kilograms:
mass of water = 750.0 g / 1000 g/kg
= 0.7500 kg
Now we can calculate the molality of the solution:
molality = moles of solute / mass of solvent (in kg)
molality = 0.267 mol / 0.7500 kg
= 0.356 mol/kg
Therefore, the molality of the solution is 0.356 mol/kg.
Determine which statements are consistent with Daltons atomic theory
Answer:
Explanation:
Dalton's atomic theory had several postulates, including:
1. All matter is made up of atoms, which are indivisible and indestructible.
2. All atoms of a given element are identical in mass and properties.
3. Compounds are formed by a combination of two or more different kinds of atoms.
4. A chemical reaction is a rearrangement of atoms.
Based on these postulates, the following statements are consistent with Dalton's atomic theory:
1. Chemical reactions involve the rearrangement of atoms to form new compounds.
2. Elements are composed of small, indivisible particles called atoms.
3. Atoms of the same element have the same mass and chemical properties.
4. A compound is made up of two or more different elements.
5. Atoms can neither be created nor destroyed in a chemical reaction.
However, the following statements are not consistent with Dalton's atomic theory:
1. Atoms are divisible into smaller particles.
2. Isotopes of the same element have different chemical properties.
3. The mass of an atom is distributed uniformly throughout the atom.
It's worth noting that while Dalton's atomic theory has been largely superseded by modern atomic theory, it remains an important historical milestone in the development of atomic theory.
when 56.6 g of calcium and 30.5g of nitrogen gas under go a reaction that has 90% yield, what mass of calcium nitride is formed?
Answer:
152.57 g
Explanation:
The balanced chemical equation for the reaction between calcium and nitrogen gas to form calcium nitride is:
3Ca + N2 → Ca3N2
From the balanced equation, we can see that the mole ratio between calcium and calcium nitride is 3:1. This means that 3 moles of calcium react to form 1 mole of calcium nitride.
First, let's calculate the number of moles of calcium and nitrogen gas given:
Mass of calcium = 56.6 g
Molar mass of calcium (Ca) = 40.08 g/mol
Moles of calcium = Mass of calcium / Molar mass of calcium = 56.6 g / 40.08 g/mol = 1.41 mol
Mass of nitrogen gas = 30.5 g
Molar mass of nitrogen gas (N2) = 28.02 g/mol
Moles of nitrogen gas = Mass of nitrogen gas / Molar mass of nitrogen gas = 30.5 g / 28.02 g/mol = 1.09 mol
Since the reaction has a 90% yield, only 90% of the limiting reactant (which is calcium in this case) will be converted to product. Therefore, we need to multiply the moles of calcium by 0.90 to account for the yield:
Moles of calcium nitride formed = Moles of calcium x Yield = 1.41 mol x 0.90 = 1.27 mol
Now, using the mole ratio from the balanced equation, we can determine the mass of calcium nitride formed:
Molar mass of calcium nitride (Ca3N2) = 40.08 g/mol (molar mass of calcium) x 3 + 14.01 g/mol (molar mass of nitrogen) x 2 = 120.25 g/mol
Mass of calcium nitride formed = Moles of calcium nitride formed x Molar mass of calcium nitride = 1.27 mol x 120.25 g/mol = 152.57 g
So, the mass of calcium nitride formed in the reaction is 152.57 g.
pls. help for chemistry hw. ASAP
6 moles will have 12 equivalents of PO₄²⁻
The mole is an amount unit similar to familiar units like pair, dozen, gross, etc. It provides a specific measure of the number of atoms or molecules in a bulk sample of matter.
A mole is defined as the amount of substance containing the same number of atoms, molecules, ions, etc. as the number of atoms in a sample of pure 12C weighing exactly 12 g.
1 mole of Mg₃(PO₄)₂ has 2 equivalents of PO₄²⁻.
Thus, 6 moles will have 2 × 6 = 12 equivalents of PO₄²⁻
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___________ is described as a metal, while __________ is described as a metalloid?
A) nitrogen, iron
B) fluorine, lithium
C) argon, sodium
D) strontium, silicon
Answer:
D) strontium, silicon
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Which of the diagrams show a beaker in which electrolysis takes place?
The beakers that we can see that electrolysis is going on are in beakers B and C
What is electrolysis?Electrolysis is a process in which an electric current is passed through a substance to produce a chemical reaction. The substance being electrolyzed is usually an electrolyte, which is a liquid or solution that contains ions.
The electric current causes the ions in the electrolyte to move towards the electrodes (conducting surfaces) where they either gain or lose electrons, depending on the nature of the electrode and the ions. This causes chemical reactions to occur at the electrodes, leading to the formation of new substances.
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Under what conditions would one mole of methane gas, ch4 , occupy the smallest volume?
Under the condition A. 273 K and 1.01 × [tex]10^{5}[/tex] Pa, one mole of methane gas, [tex]CH_{4}[/tex], occupy the smallest volume.
What is the smallest volume ?
The ideal gas law, PV = nRT, can be rearranged to solve for volume as V = nRT/P, where V is volume, n is the number of moles, R is the gas constant, T is temperature in Kelvin, and P is pressure.
To find the conditions under which one mole of methane gas occupies the smallest volume, we need to find the combination of temperature and pressure that results in the smallest volume.
Using the equation V = nRT/P, we can see that volume is inversely proportional to pressure, so we want the highest pressure possible. Therefore, we can eliminate choices A and C, which have lower pressures than B and D.
Next, we need to consider temperature. Using the same equation, we can see that volume is directly proportional to temperature, so we want the lowest temperature possible. Therefore, the correct choice is A, which has a temperature of 273 K, the lowest temperature of all the choices.
Therefore, the answer is A. 273 K and 1.01 × [tex]10^{5}[/tex] Pa.
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Complete question is: Under the 273 K and 1.01 × [tex]10^{5}[/tex] Pa condition, one mole of methane gas, [tex]CH_{4}[/tex], occupy the smallest volume.
What is the molarity of an unknown H2C2O4 solution if 10.00 mL of the H2C2O4 solution required 15.85 mL of 0.0198 M KMnO4 solution to obtain a stoichiometric endpoint?
2 KMnO4 + 5 H2C2O4 + 3 H2SO4 → 2 MnSO4 + 10 CO2 + K2SO4 + 8 H2O
Answer:
Explanation:
to balance the given chemical equation using the oxidation state change method, we need to follow these steps:Step 1: Write the unbalanced equationKMnO4 + KCl + H2SO4 → K2SO4 + MnSO4 + Cl2Step 2: Identify the elements that undergo oxidation and reductionIn this equation, the oxidation state of Mn changes from +7 to +2, which means it undergoes reduction, while the oxidation state of Cl changes from -1 to 0, which means it undergoes oxidation.Step 3: Write the half-reactionsReduction half-reaction: MnO4^- → Mn^2+Oxidation half-reaction: Cl^- → Cl2Step 4: Balance the atoms and charges in each half-reactionReduction half-reaction: 8H+ + MnO4^- → Mn^2+ + 4H2OOxidation half-reaction: 2Cl^- → Cl2 + 2e^-Step 5: Balance the electrons in each half-reactionReduction half-reaction: 5e^- + 8H+ + MnO4^- → Mn^2+ + 4H2OOxidation half-reaction: 2Cl^- → Cl2 + 2e^-Step 6: Multiply each half-reaction by a factor to equalize the number of electrons transferredReduction half-reaction: 10e^- + 16H+ + 2MnO4^- → 2Mn^2+ + 8H2OOxidation half-reaction: 14Cl^- → 7Cl2 + 14e^-Step 7: Add the balanced half-reactions together10e^- + 16H+ + 2MnO4^- + 14Cl^- → 2Mn^2+ + 8H2O + 7Cl2Step 8: Cancel out the common terms on both sides of the equation2KMnO4 + 16KCl + 8H2SO4 → 2K2SO4 + 2MnSO4 + 7Cl2 + 8H2OTherefore, the balanced equation using the oxidation state change method is:2KMnO4 + 16KCl + 8H2SO4 → 2K2SO4 + 2MnSO4 + 7Cl2 + 8H2O.
A researcher is studying gold complexes. She makes
a 125 mL solution of gold(III) chloride by dissolving
0.144 moles of the solute into water. Which of the
following would cause the concentration of the
solution to increase?
Additional gold(III) chloride is added to the
beaker.
Part of the solution is poured into the chemical
waste.
O Water is added to the beaker.
We do not have enough information to answer
this question.
Additional gold(III) chloride is added to the beaker. This would cause the concentration of the solution to increase. Therefore, the correct option is option A.
Concentration in chemistry refers to the quantity of a material in a certain area. The ratio of the solute within a solution to the solvent or whole solution is another way to define concentration. In order to express concentration, mass / unit volume is typically used.
The solute concentration can, however, alternatively be stated in moles or volumetric units. Concentration may be expressed as per unit mass rather than volume. Although concentration is typically used to describe chemical solutions, it may be computed for any mixture. Additional gold(III) chloride is added to the beaker. This would cause the concentration of the solution to increase.
Therefore, the correct option is option A.
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6) Apply the rules for canceling complex units to simplify and find the units in an answer:
a)
=
atm / mol • (atm •L/
mol • K)
b) (mol • (atm•L / mol • K) • K ) / L
Cancelling units, also referred to to be "unit analysis" as well as "dimensional analysis," atm / mol × (atm ×L/mol × K) = atm / (atm ×L/ K)
A conversion factor (described in the form of a fractions, ) is considered as possessing a value of "1" for the purposes of transforming between units. Cancelling units, also referred to to be "unit analysis" as well as "dimensional analysis," depends on the principles that multiplying a thing by "1" does not alter the value, that any amount divided through a single value equals "1," and that any value allocated by itself.
A) atm / mol × (atm ×L/mol × K)
cancel the mole by mole
atm / (atm ×L/ K)
B) (mol × (atm×L / mol × K) × K ) / L
cancel the mole by mole
(atm×L / K) × K ) / L
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A 346.9 mL sample of carbon dioxide was heated to 373 K. If the volume of the carbon dioxide sample at 373 K is 596.2 mL,
what was its temperature at 346.9 mL?
T =
Answer:
216.9 K
Explanation:
We can use the combined gas law to solve this problem:
(P1V1/T1) = (P2V2/T2)
where P is pressure, V is volume, and T is temperature. We can assume that the pressure is constant, since the problem doesn't mention any changes in pressure.
Let's label the initial temperature T1 and the final temperature T2, and plug in the given values:
(P1V1/T1) = (P2V2/T2)
V1 = 346.9 mL
V2 = 596.2 mL
T2 = 373 K
(P1 * 346.9 mL / T1) = (P1 * 596.2 mL / 373 K)
Simplifying and solving for T1:
T1 = (P1 * 346.9 mL * 373 K) / (P1 * 596.2 mL)
T1 = (346.9 * 373) / 596.2
T1 = 216.9 K
Therefore, the temperature of the carbon dioxide sample at 346.9 mL was 216.9 K.
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Show that the following reaction obeys zero order kinetics, and find the rate constant and half-life. 10²x[A]/mol dm-3 13.80 11.05 8.43 5.69 3.00 Time/hr 0 10 20 30 40
The half life for the given reaction is 20s. The rate constant for the given zero order reaction can be given as 0.5mol L⁻¹s⁻¹.
According to the definition of a zero-order reaction, it is "a chemical reaction that occurs when the rate of response remains unchanged whether the percentage of the reactants increases or decreases." Since the rate increases according in proportion to the 0th magnitude of the reactant concentration, the rate at which these responses is always equivalent to the constant rate for the particular reactions.
k = 0.5mol L⁻¹s⁻¹
Half life is a/2K=3/2×40
= 20s
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1. A new 125 g alloy of brass at 100°C is dropped into 76 g of water at 25 "C The final temperature of the water and brass is 35 "C. what is the specific heat of the sample of brass? The specific heat of water - 4.184 J/g.
We can solve this problem using the principle of conservation of energy, which states that the total energy of an isolated system remains constant.
The heat lost by the brass is equal to the heat gained by the water:
heat lost by brass = heat gained by water
The heat lost by the brass can be calculated as:
Qbrass = mbrass × cbrass × ΔT
where mbrass is the mass of the brass, cbrass is its specific heat, and ΔT is the change in temperature of the brass.
The heat gained by the water can be calculated as:
Qwater = mwater × cwater × ΔT
where mwater is the mass of the water, cwater is its specific heat, and ΔT is the change in temperature of the water.
Since the brass and water reach a final temperature of 35°C, we know that:
ΔT = Tfinal - Tinitial = 35°C - 25°C = 10°C
Plugging in the given values, we get:
Qbrass = mbrass × cbrass × ΔT = (0.125 kg) × cbrass × (10°C) = 1.25 cbrass J
Qwater = mwater × cwater × ΔT = (0.076 kg) × (4.184 J/g°C) × (10°C) = 31.97 J
Since Qbrass = Qwater, we can set the two equations equal to each other and solve for cbrass:
1.25 cbrass J = 31.97 J
cbrass = 31.97 J / 1.25 J/kg°C = 25.58 J/kg°C
Therefore, the specific heat of the brass sample is 25.58 J/kg°C.
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Watch the animation and select the interactions that can be explained by hydrogen bonding.
HF
is a weak acid neutralized by NaOH
.
HF
has a higher boiling point than HCl
.
CH4
molecules interact more closely in the liquid than in the gas phase.
Ice, H2O
, has a solid structure with alternating H−O
interactions.
H2Te
has a higher boiling point than H2S
The interactions that can be explained by hydrogen bonding are:
HF has a higher boiling point than HClIce, H₂O, has a solid structure with alternating H−O interactions.Hydrogen bonding is a type of intermolecular force that occurs between a hydrogen atom in a polar molecule and a highly electronegative atom, such as nitrogen, oxygen, or fluorine, in a neighboring molecule. It is a relatively strong force and can significantly affect the physical and chemical properties of substances.
In the case of HF and HCl, both molecules are polar, but HF has a higher boiling point due to the stronger hydrogen bonding between its molecules. In ice, the hydrogen bonding between water molecules creates a crystal structure with a characteristic lattice arrangement.
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Calculation: 3. A new alloy of steel is 525 g at 100-C. It is dropped into 375 grams of water at 25 C. The final temperature changes to 55C, what is the specific heat of steel?
The specific heat capacity of the steel is 2 g/°C.
What is the specific heat capacity of the steel?To determine the specific heat capacity of a particular sample of steel, the sample can be heated to a known temperature and then placed in contact with a known amount of water at a lower temperature.
We know that the heat lost by the steel is equal to the heat gained by the water.
Thus we have that;
-(525 * c * (55- 100)) = (375 * 4.2 * (55- 25)
23625c = 47250
c = 47250/23625
c = 2 g/°C
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A compound contains 0.58 m Ag, 0.58 mol N, and 1.79 mol O. What is its empirical formula?
Explanation:
To find the empirical formula of the compound, we need to determine the simplest whole-number ratio of the atoms in the compound.
First, we need to find the number of moles of Ag, N, and O relative to each other. The smallest number of moles is used as a reference point, and the other moles are divided by this value to get their ratios:
0.58 mol Ag : 0.58 mol N : 1.79 mol O
Dividing each mole value by 0.58 mol (the smallest number of moles), we get:
1 mol Ag : 1 mol N : 3.09 mol O
We can see that the ratio of Ag:N:O is 1:1:3.09. However, we need to express the ratio in whole numbers, so we divide each number by the smallest number in the set of ratios:
1 : 1 : 3.09/1.00 ≈ 3.
Rounding to the nearest whole number, we get the empirical formula of the compound:
AgN3O3
Therefore, the empirical formula of the compound is AgN3O3.
Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte.
(a) PbCl2
(b) N(CH3)3
(c) CsOH
(d) H2S
(e) CrCl2
(f) Ni(CH3COO)2
Strong electrolyte: lead(II) chloride weak electrolyte trimethylamine Strong electrolyte: cesium hydroxide sulphide of hydrogen: a weak electrolyte, strong electrolyte chromium chloride Weak electrolyte: nickel(II) acetate
Is acetic acid an electrolyte that is weak?Response and justification The fact that acetic acid has a low dissociation constant suggests that it is a weak acid. Acetic acid's restricted ability to ionise in an aqueous solution is a result of its low dissociation constant. With this in mind, acetic acid can be regarded as a weak electrolyte.
Is acid phosphoric a type of electrolyte?Phosphoric acid is a useful electrolyte because of its low volatility, strong ionic conductivity, stability at high temperatures, carbon dioxide and carbon monoxide tolerance, and low flammability.
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Calculate the mass of water produced when 1.03 g
of butane reacts with excess oxygen.
1.03 g of butane will yield 1.59 g of water when it reacts with too much oxygen.
What is mass?The amount of matter in an item is measured by the fundamental physical quantity known as mass. It is a scalar quantity that is measured in grams (g) or kilograms (kg) (g). No matter where it is or what force is pushing against it, an object's mass always remains constant.
How do you determine it?For butane and oxygen to burn, the chemical equation is balanced as follows:
2C4H10+13 O2→ 8 CO2+ 10 H2O
According to the equation, 1 mole of butane (C4H10) and 13/2 moles of oxygen (O2) combine to form 5 moles of water (H2O).
To begin with, we must count the butane moles that are present:
Mass of butane divided by its molar mass yields moles of butane.
1.03 g/58.12 g/mol is the formula for butane.
A mole of butane weighs 0.0177 mol.
Then, we can calculate the quantity of water created using the butane-to-water mole ratio:
Moles of water = [tex]\frac{5 mol H2O}{(1 mol C4H10 ×0.0177 mol C4H10)}[/tex] = 0.0885 mol.
Eventually, we can determine how much water was generated:
moles of water equal 0.0885 mol when 5 mol H2O is divided by 1 mol C4H10 and multiplied by 0.0177 mol C4H10.
Lastly, we can determine the mass of created water:
Water's mass is equal to its moles times its molar mass= 0.0885 mol × 18.02 g/mol = 1.59 g.
As a result, 1.03 g of butane will yield 1.59 g of water when it reacts with to moles of water equal 0.0885 mol when 5 mol H2O is divided by 1 mol C4H10 and multiplied by 0.0177 mol C4H10.
Lastly, we can determine the mass of created water:
Water's mass is equal to its moles times its molar mass = 0.0885 mol × 18.02 g/mol = 1.59 g.
As a result, 1.03 g of butane will yield 1.59 g of water when it reacts with too much oxygen.
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Consider a sample containing 0.300 mol of a substance. How many atoms are in the sample if the substance is iron?
The number of atoms in a sample containing 0.300 mol of iron is 1.8066 x 10²³ atoms.
The number of atoms in a sample of a substance can be determined using Avogadro's number, which is equal to 6.022 x 10²³ particles per mole. The atomic mass of iron is 55.85 g/mol.
Therefore, 0.300 mol of iron will contain:
0.300 mol x 6.022 x 10³ atoms/mol = 1.8066 x 10²³ atoms
Avogadro's number is a fundamental constant in chemistry that represents the number of particles (atoms or molecules) in one mole of a substance.
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What is the temperature of 0.59 mol of gas at a pressure of 1.0 atm and a volume of 11.0 L? (Express the temperature in kelvins to two significant figures).
Answer:
T = 230 K
Explanation:
Simply use the equation: PV = nRT, where P is pressure, V is volume, n is moles, R is 0.0821, and T is temperature in kelvin
Place the values in
(1.0 atm)(11.0 L)=(0.59 moles)(0.0821 Lxatm/Kxmol)(T)
Solve for T = 230 K