1. The number of molecules in 1 atm of gas at constant pressure and temperature
ID: 856412 • Letter: 1
Question
1. The number of molecules in 1 atm of gas at constant pressure and temperature is identical, regardless of the identity of the molecules in the gas. Which of the following other statements are also true?
A) The molecules in a gas slow down with increasing temperature.
B) The total number of atoms in the gas at standard temperature and pressure can vary depending on the identity of the gas
C) The volume of a gas is independent of the pressure of the gas.
D) The temperature of a gas is independent of the pressure of the gas.
2. In an ideal gas, P*V = n*R*T where P = pressure, V=volume, n=number of moles, R=gas constant, and T=temperature. Consider a gas with pressure = 1 atm, 1 mole of molecules, and a temperature of 295 K. R=0.082 atm*L/(mol * K). How much volume should this gas occupy? Choose the closest answer.
A) 1.0 L
B) 30.6 L
C) Infinite space
D) 22.4 L
3. Suppose you conducted an experiment using Helium gas. Given that Helium is much lighter than Propane and Butane, you would expect the relationship between the volume of helium and the pressure to be:
A) exponential, because Helium is lighter
B) inversely proportional, just like propane and butane
C) directly proportional, just like propane and butane
D) periodic, because Helium is lighter
4. What do you predict would happen if you conducted an experiment using sulfur hexafluoride (SF6) which is much heavier than methane or butane?
A) The volume of SF6 would be larger and this would affect the pressure in the flask
B) The relationship between temperature and volume would be inversely proportional for a gas of higher molecular weight
C) The speed of the SF6 gas molecules would be faster causing a difference in the temperature measurements
D) The relationship between temperature and volume would be directly proportional just as it was for methane and butane
Explanation / Answer
1) B
2) 22.4( from the given values we will get 24.19L)
3) B
4) D
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