# Chapter 5 - Gases - Questions: 32

a. True b. False. At constant temperature, the weight of gas molecules is independent of the average kinetic energy of the gas molecules. c. True d. False. as temperature increases, the effect of interparticle interactions on gas behavior is decreased. e. True f. False. The kinetic molecular theory predicts that pressure is directly proportional to temperature at constant volume and moles of gas.

#### Work Step by Step

a. Given the formula for kinetic energy = $0.5mv^2$, a lighter mass corresponds to a faster velocity. b. Temperature is a measure of the average kinetic energy. Therefore, if the temperature is constant, there should be no variation on average kinetic energy based on the weight of atoms. c. If the container is large, the particles will be able to move around more freely and at faster speeds. Therefore, intermolecular forces are minimized in these free-moving conditions. d. If the temperature is increased, particles experience greater velocities and motion. As a result, intermolecular interactions are minimized at such high speeds. e. With a greater number of molecules, a greater number of collisions occur against the container wall and therefore a greater pressure. f. We rearrange the ideal gas law to find that $P=\frac{nRT}{V}$. Here, we see that pressure is instead directly proportional to temperature.

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