A Which of the following is not an assumption of the Kinetic

A. Which of the following is not an assumption of the Kinetic Molecular Theory of Gases? a. Gases have a negligible volume b. Gases are in constant motion and do not lose energy c. Gases do not affect each other d. Average kinetic energy is proportional to temperature for any gas e. Gases of a certain pressure all have the approximate same speed B. Which gas has the highest density? a. He b. CH4 c. NH3 d. C12 e. none of the above C. A gaseous mixture containing 1.5 moles of Argon and 3.5 moles of carbon dioxide has a total pressure of 7.0 atm. What is the mixture partial pressure of carbon dioxide? a. 1.8 atm b. 2.1 atm c. 2.4 atm d 3.5 atm e. 4.9 atnm D. If the volume of a container containing a gas is doubled and the pressure (in tort) is also then the resulting temperature: a. remains the same b. increases c. decreases E. Given the reaction 2NH, + 3C12 N, + 6HCI , you react 5.0 L of NH, with 5.0 L of Cl. (measured under the same conditions in a closed container). Calculate ratio of pressures in the container (PP a. 0.75 L b. 1.00 L c. 1.33 L d. 1.50 L e. None of these

Solution

A) option e

According to kinetic theory of gases all gas molecules at a given pressure do not have same speed, but different speeds.

B) option d

The higher the molar mass, higher is the density , as molar mass is proportional to density.

Thus Cl2 gas with highest molar mass(71g/mol) is the one with highest density.

C) Option e

Argon 1.5 moles and CO2 3.5moles

total pressure = 7.0 atm

We know from Daltons law of partial pressures,

partial pressure of a gas = its mole fraction x total pressure

Thus

mole fraction of CO2 = 3.5/(3.5+1.5)

partial pressure of CO2 = [ 3.5/5] x 7 atm

= 4.9 atm

D) option B

From ideal gas equation

PV = nRT

as both pressure and volume are doubled, the temperature also increases by 4 fold.(as number of moles and R are constant)