Which of the following statements are true? A.The number of moles in 1.00 atm of gas was the same, despite the fact that the gases themselves had different identities. B.The number of moles in 1.00 atm of gas varied linearly with increasing molar mass. C.The volume of the gas varied depending on the identity of the gas. D.The number of moles in 1.00 atm of gas varied hyperbolically with increasing molar mass.
Given Avogadro's Law, which of the following statements are true? A.The number of molecules in a gas increases with temperature. B.The total number of atoms in a gas at STP 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.
In this experiment, the pressure of the gas was 1.00 atm and the temperature was 294.6 K. What value do you get for the gas constant using the data you recorded for propane? A.1.858 L atm mol-1 K-1 B.0.0008 L atm mol-1 K-1 C.0.0820 L atm mol-1 K-1 D.81.991 L atm mol-1 K-1
How many moles of methane were in the Erlenmeyer flask? A.1.72 × 10-3 mol B.6.23 × 10-3 mol C.6.23 × 10-2 mol D.2.26 × 10-3 mol
How many molecules of propane were in the Erlenmeyer flask? Avogadro's number is 6.022 × 1023 molecules/mol. A.6.022 × 1023 molecules B.3.74 × 1023 molecules C.7.50 × 1021 molecules D.3.74 × 1021 molecules
Suppose you have a mixture of ideal gases. Which of the following statements is false A.The gases will expand to fill the entire container. B.The total pressure is equal to the sum of partial pressures of the constituent gases. C.The mixture will behave as an ideal gas to a first approximation. D.The molar volume depends on the identity of the gases.
1) Option A. The moles of an ideal gas do not depend on your identity.
2) Option B. The total number of atoms depends on the identity of the gas.
3) Option C. The correct value of the constants is 0.082 atm * L / mol * K
4) The moles are calculated:
n = P * V / R * T = 1 atm * 0.15 L / 0.082 atm * L / mol * K * 294.6 K = 6.23x10 ^ -3 mol
5) Molecules are calculated:
molecules = n * NA = 6.23x10 ^ -3 * 6.02x10 ^ 23 = 3.74x10 ^ 21 molecules
6) The false option is D. The molar volume does not depend on the identity of the gases.
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