A sample of helium gas, He(g), is placed in a rigid cylinder sealed with a movable piston.
The temperature of the helium is 25.0°C. The volume of the helium is 300. milliliters and
the pressure is 0.500 atmosphere.

16) State, in terms of the average distance between the helium atoms, why the density of the gas increases when the piston is pushed farther into the rigid cylinder. [1]

17) Determine the volume of the helium gas when the pressure is increased to 1.50 atm and
the temperature remains at 25.0°C. [1]

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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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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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.

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

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.

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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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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Okay, here are the steps to solve this problem:

a) To neutralize 15ml of 0.10 mol/L sodium carbonate solution, the hydrochloric acid solution must contain 0.015 moles of HCl.

Since the HCl solution is made by dissolving HCl gas in 100ml water, we can calculate the moles of HCl gas dissolved in 100ml:

0.015 moles HCl / 15ml sodium carbonate solution = X moles HCl gas / 100ml HCl solution

X = 0.015 * (100/15) = 0.01 moles HCl gas

b) Molar volume of HCl gas at STP is 24.45 L/mol.

So the volume of 0.01 moles HCl gas is: 0.01 moles * 24.45 L/mol = 0.2445 L

Since the solution is made with this gas in 100ml water, the volume of HCl gas dissolved in 100ml water is 0.2445 L.

So the final answers are:

a) 0.01 moles of HCl gas

b) 0.2445 L of HCl gas

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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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Answer:

Explanation:

Use the Equation: [tex]\frac{V1}{T1}=\frac{V2}{T1} \\[/tex]

V1 = 346.9 mL

T1 = ? K

V2 = 596.2 mL

T2 = 373 L

This assumption can only be made when pressure is held constant.

[tex]\frac{346.9}{V1}=\frac{596.2}{373}, solve for V1\\ V1 = 217.0 K[/tex]

The interactions that can be explained by hydrogen bonding are:

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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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.

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.

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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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.

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Problem 1:

The osmotic pressure (π) can be calculated using the van 't Hoff equation: π = iMRT, where i is the van 't Hoff factor (1 for water), M is the molar concentration, R is the gas constant, and T is the temperature in Kelvin.

In this case, the molar concentration is 1.13 mol/L, and the temperature is 25°C = 298 K. So,

π = iMRT = (1)(1.13 mol/L)(0.08206 L·atm·K⁻¹·mol⁻¹)(298 K)

π = 29.8 atm

Therefore, a pressure of 29.8 atm must be applied to prevent osmotic flow of pure water into sea water through a membrane permeable only to water molecules at 25°C.

Problem 2:

The osmotic pressure of a solution can be calculated using the van 't Hoff equation: π = iMRT, where i is the van 't Hoff factor, M is the molar concentration, R is the gas constant, and T is the temperature in Kelvin.

First, we need to find the molar concentration of glucose in the solution. The molecular weight of glucose is 180.16 g/mol. So,

Molar concentration = (mass/volume) / (molecular weight)

Molar concentration = (6.65 g/0.35 L) / 180.16 g/mol

Molar concentration = 0.104 mol/L

Now, we can calculate the osmotic pressure:

π = iMRT = (1)(0.104 mol/L)(0.08206 L·atm·K⁻¹·mol⁻¹)(308 K)

π = 2.44 atm

Therefore, the osmotic pressure of the solution prepared by adding 6.65 g of glucose to enough water to make 350 mL of solution at 35°C is 2.44 atm.

Problem 3:

Using the same process as in Problem 2, we can find the molar concentration of glucose in the solution:

Molar concentration = (mass/volume) / (molecular weight)

Molar concentration = (9.0 g/0.45 L) / 180.16 g/mol

Molar concentration = 0.44 mol/L

Now, we can calculate the osmotic pressure:

π = iMRT = (1)(0.44 mol/L)(0.08206 L·atm·K⁻¹·mol⁻¹)(308 K)

π = 10.2 atm

Therefore, the osmotic pressure of the solution prepared by adding 9.0 g of glucose to enough water to make 450 mL of solution at 35°C is 10.2 atm.

Problem 4:

Propanol (C₃H₇OH) is a non-electrolyte, so its van 't Hoff factor is 1.

First, we need to find the molar concentration of propanol in the solution. The molecular weight of propanol is 60.10 g/mol. So,

Molar concentration = (mass/volume) / (molecular weight)

Molar concentration = (11.0 g/0.85 L) / 60.10 g/mol

Molar concentration = 0.178 mol/L

Now, we can calculate the osmotic pressure:

π = iMRT = (1)(0.178 mol/L)(0.08206 L·atm·K⁻¹·mol⁻¹(298 K)

π = 3.67 atm

Therefore, the osmotic pressure of the solution prepared by adding 11.0 g of propanol to enough water to make 850 mL of solution at 25°C is 3.67 atm.

Problem 5:

Using the same process as in Problem 2 and Problem 3, we can find the molar concentration of glucose in the solution:

Molar concentration = (mass/volume) / (molecular weight)

Molar concentration = (65 g/35,000 mL) / 180.16 g/mol

Molar concentration = 0.00177 mol/L

Now, we can calculate the osmotic pressure:

π = iMRT = (1)(0.00177 mol/L)(0.08206 L·atm·K⁻¹·mol⁻¹)(288 K)

π = 0.0398 atm

Therefore, the osmotic pressure of the solution prepared by adding 65 g of glucose to enough water to make 35,000 mL of solution at 15°C is 0.0398 atm.

1.03 g of butane will yield 1.59 g of water when it reacts with too much oxygen.

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.

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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Answer:

1) -572 kJ/mol

2) -2220.7 kJ/mol

Explanation:

Multiply the bond enthalpies to take into account the amount of moles of each compound in the reaction. Then, to get the total change in energy/enthalpy in the reaction, subtract the reactant energy from the product energy.

1) 2(-286) = -572 kJ/mol

2) 4(-286) + -393.5(3) - -103.8 = -2220.7 kJ/mol

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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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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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.

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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.

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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A percentage expressing the variation between a calculated/measured value and the anticipated/real value is known as a "calculated percent error."

A positive numerical discrepancy implies that the assessed number exceeds what was expected, with negative values indicating the reverse.

When conducting an experiment, if an excessive percent error emerges it suggests potential errors or miscalculations in experimental design, data collection, or analysis.

This may mean unaccounted variables were present, and equipment/procedures require refinement. In opposition, lower percentages signal accuracy despite any limitations resulting from the human elements involved.

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ΔH° = ΔHf° is true for two reactions which are ,

H₂(g) + S(rhombic) → H₂S(g)

C(diamond) + O₂(g) → CO₂(g)

Hence, option a and b are correct.

∆Hf is the enthalpy of formation, is the enthalpy when product is made from its constituent elements. Generally the enthalpy of formation is described as the standard reaction enthalpy for the formation of the compound from its elements (which may include atoms or molecules) in their most stable reference states at the chosen temperature (298.15K) and at 1bar pressure.

In a part, H₂S is formed by H₂ and S means it's constituent elements.

So, a is correct.

In b also, CO₂ is formed by C and O₂, so b is also correct. Hence, option a and b are correct.

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In 15.0 mL of a 2.5 molar magnesium chloride solution, there are approximately 4.51 × 10^{22} chloride ions.

An inorganic compound composed of one magnesium ion and two chloride ions.

We must first determine the number of moles of MgCl_2 in the solution,

moles of solute = concentration × volume (in liters)

Converting the solution's volume from milliliters to liters,

15.0 mL = 15.0 × 10^{-3} L

moles of MgCl_2 = 2.5 mol/L × 15.0 × 10^{-3} L = 0.0375 moles

The solution contains the following number of chloride ions:

number of Cl^{-} ions = 2 × moles of MgCl_2

Substitute the value of moles of MgCl_2,

number of Cl^{-} ions = 2 × 0.0375 moles = 0.075 moles

by using Avogadro's number:

number of Cl^{-} ions = 0.075 moles × 6.02 × 10^{23} ions/mol ≈ 4.51 × 10^{22} ions

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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.

The specific heat capacity of the steel is 2 g/°C.

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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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

The beakers that we can see that electrolysis is going on are in beakers B and C

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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