Question 1

What is Avogadro's law? Explain.

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Question 2

What is pressure? How is it calculated?

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Question 3

Explain the concept of ideal gas law.

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Question 4

A container has a mixture of H₂ at 1.2 atm and O₂ at 1.6 atm. What is the mole fraction of H₂?

Accepted Answer

The mole fraction of a gas is the ratio of its partial pressure to the total pressure. Total pressure = 1.2 atm + 1.6 atm = 2.8 atm. Mole fraction of H₂ = 1.2 atm / 2.8 atm = 0.43.

Question 5

Which of the following statements is consistent with the Dalton's law of partial pressures?

Accepted Answer

Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases in the mixture.

Question 6

Briefly explain Dalton's law of partial pressures.

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Question 7

What are the postulates of the kinetic theory of gases?

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Question 8

What is molar volume? What is the molar volume of gases at STP

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Question 9

Briefly explain Boyle's law.

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Question 10

What is the combined gas law?

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Question 11

Briefly describe Gay-Lussac's law. Highlight the difference between Gay-Lussac's and Charles's law.

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Question 12

A mixture of helium at 1.600 atm and neon at 900.0 torr is in a container. What is the total pressure in the container?

Accepted Answer

To find the total pressure, convert helium's pressure from atm to torr: 1.600 atm = 1.600 x 760 torr = 1216 torr. Add this to neon's pressure: 1216 torr + 900 torr = 2116 torr.

Question 13

What are ideal gases? Can real world gases be called ideal gases?

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Question 14

Briefly explain Charles's law.

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Question 15

Explain the concept of standard temperature and pressure.

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Question 16

Explain the significance and use of the ideal gas law.

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Question 17

H₂ stored in a 50.0 L container has a pressure of 500.0 torr. O₂ stored in a 25.0 L container has a pressure of 800.0 torr. If both these gases are released together to be stored in a 100.0 L container, what is the total pressure in the 100.0 L container?

Accepted Answer

The total pressure can be found using the ideal gas law and the principle of partial pressures. First, calculate the moles of each gas using $P_1V_1 = nRT$ (where $R$ and $T$ are constants and can be ignored for this calculation since they are the same for both gases and the process). For the first gas: $n_1 = \frac{P_1V_1}{RT} = \frac{500 \times 50}{RT}$. For the second gas: $n_2 = \frac{P_2V_2}{RT} = \frac{800 \times 25}{RT}$. When combined in a 100.0 L container, the total moles $n_{total} = n_1 + n_2$. The total pressure $P_{total}$ can then be found using $P_{total}V_{total} = n_{total}RT$, where $V_{total} = 100.0 L$. Simplifying, we find $P_{total} = \frac{(500 \times 50 + 800 \times 25)}{100}$ torr = 450 torr.

Question 18

CO₂ generated by the decomposition of ZnCO₃, is collected in a 5.6 L container over water. If the temperature is 40.0°C and the total pressure inside the container is 580 torr, how many moles of CO₂ were generated?

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Question 19

What are the various units of pressure? Show how to convert one pressure unit into another using dimensional analysis. The formal, SI-approved unit of pressure is the pascal (Pa), which is defined as 1 N/m². A common unit of pressure is the atmosphere (atm), which was originally defined as the average atmospheric pressure at sea level. A more reliable and common unit is millimeters of mercury (mmHg), which is the amount of pressure exerted by a column of mercury exactly 1 mm high. An equivalent unit is the torr, which equals 1 mmHg. 1.00 atm

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Question 20

A mixture of H₂ at 566 torr and O₂ at 600 torr is in a container. What is the total pressure in the container?

Accepted Answer

The total pressure in a mixture of gases is the sum of the partial pressures of the individual gases. Therefore, the total pressure is 566 torr (from HS) + 600 torr (from OS) = 1,166 torr.

Quiz 6: Gases