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### 4. Gases in order of rate of effusion - a. List the following gases in order of rate of effusion, from lowest to highest. (Assume all gases are at the same temperature and pressure.) - He - Xe - Cl₂ - HCl - b. Explain why you put the gases in the order above. Refer to the ki...

### 4. Gases in order of rate of effusion - a. List the following gases in order of rate of effusion, from lowest to highest. (Assume all gases are at the same temperature and pressure.) - He - Xe - Cl₂ - HCl - b. Explain why you put the gases in the order above. Refer to the kinetic-molecular theory to support your explanation. - Because effusion depends on atomic mass, and according to the kinetic molecular theory, gases that are lighter have a higher effusion rate. ### 5. Polar vs. Nonpolar gases - Explain why polar gas molecules experience larger deviations from ideal behavior than nonpolar molecules when all other factors (mass, temperature, etc) are held constant. - Because they have strong attractive forces, which is the opposite of the assumption of the kinetic molecular theory. ### 6. Simultaneous injection of gases - The two gases in the figure below are simultaneously injected into opposite ends of the tube. The ends are then sealed. They should begin to mix closest to which labeled point? - (c) ### 7. Speed-distribution curves - Explain the difference in the speed-distribution curves of a gas at the two temperatures shown in the figure below. - As the temperature increases, molecular speed increases.