Question 1

Which of the following compounds will behave least like an ideal gas at low temperatures?

Accepted Answer

The compound CCl₄ (carbon tetrachloride) has strong intermolecular forces due to its polar bonds and lack of symmetry, which make it less likely to behave like an ideal gas at low temperatures. The other compounds listed are either noble gases (Ar, Kr) or diatomic molecules with relatively weak intermolecular forces (O2, F2).

Question 2

Why does the rate of effusion increase with a decrease in the molar mass?

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Question 3

Give the major gas in dry air.

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Question 4

Calculate the ratio of effusion rates of Cl₂ to F₂.

Accepted Answer

The effusion rate is inversely proportional to the molecular weight of the gas. The molecular weights of Cl₂ and F₂ are approximately 98 and 88, respectively. Ratio of effusion rates = sqrt(Molecular weight of F₂) / sqrt(Molecular weight of Cl₂) = sqrt(88) / sqrt(98) ≈ 0.732. Therefore, the correct answer is E.

Question 5

Identify the element or molecule with the highest van der Waals constant.

Accepted Answer

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Question 6

Identify the element or molecule that has the highest effusion rate.

Accepted Answer

The effusion rate of a gas is inversely proportional to the square root of its molar mass (Graham's law). Helium (He) has the lowest molar mass among the given options, thus it will have the highest effusion rate.

Question 7

The rate of effusion of oxygen to an unknown gas is 1.49.What is the other gas?

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Question 8

Why doesn't Dalton's Law of Partial Pressures depend on the identity of the gases present?

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Question 9

Identify the element or molecule that has the highest diffusion rate.

Accepted Answer

Hydrogen (H₂) has the smallest molecular weight among the given options, leading to the highest diffusion rate according to Graham's law of effusion and diffusion.

Question 10

If CO₂ and NH₃ are allowed to effuse through a porous membrane under identical conditions,the rate of effusion for NH₃ will be ________ times that of CO₂.

Accepted Answer

The rate of effusion is inversely proportional to the square root of the molar mass. The molar mass of CO₂ is approximately 56 g/mol and the molar mass of NH₃ is approximately 46 g/mol. Thus, the square root of the ratio of their molar masses is approximately 0.83. Therefore, the rate of effusion for NH₃ will be approximately 1.2 times that of CO₂. Rounded to one significant figure, the answer is 1.6.

Question 11

Identify the element or molecule that has the lowest effusion rate.

Accepted Answer

The effusion rate is inversely proportional to the molecular weight of the substance. Xe has the highest molecular weight among the options given and therefore has the lowest effusion rate.

Question 12

Why does HOT air rise?

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Question 13

Define pressure.

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Question 14

Rank the following in order of decreasing rate of effusion. F₂ SF₆ Ne Kr

Accepted Answer

The rate of effusion of gases is inversely proportional to the square root of their molar masses (Graham's law). Ne (Neon) is the lightest, followed by F₂ (presumably a lighter compound), then Kr (Krypton), and finally SF₆ (presumably the heaviest compound). This order reflects decreasing rates of effusion.

Question 15

Consider a container of gas under a particular P,V,T set of conditions.Describe how the pressure would change if the volume were doubled while the absolute temperature was increasing by a factor of two.

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Question 16

A sample of N₂ effuses in 200 s.How long will the same size sample of Cl₂ take to effuse?

Accepted Answer

Graham's law of effusion states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. The formula to compare the effusion times of two gases is $t_1 / t_2 = \sqrt{M_2 / M_1}$, where $t_1$ and $t_2$ are the effusion times, and $M_1$ and $M_2$ are the molar masses of the gases. The molar mass of N₂ (N2S) is 46 g/mol, and the molar mass of Cl₂ (Cl2S) is 102.97 g/mol. Plugging these values into the formula, we get $200 / t_2 = \sqrt{46 / 102.97}$, solving for $t_2$ gives approximately 318 seconds.

Question 17

Given the equation C₂H₆(g)+ O₂(g)→ CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of O₂ consumed at STP when 150.0 grams of C₂H₆ is burned.

Accepted Answer

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Question 18

Explain what the term "mean free path" describes.How does it change with decreasing pressure?

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Question 19

Given the equation C₂H₆(g)+ O₂(g)→ CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of CO₂ formed at STP when 120.0 grams of C₂H₆ is burned in excess oxygen gas.

Accepted Answer