Using kinetic-molecular theory, explain why pressure and moles are directly proportional, i.e. why an increase in the number of moles leads to an increase in pressure. Be sure to address kinetic energy and number of collisions between molecules

The volume of a gas will increase when I. The pressure of the gas increases. II. The number of moles of the gas increases. III. The temperature of the gas increases.       II only     I only     III only     I, II, and III     II and III

Consider a 1.0-L container of neon gas at STP. Will the average kinetic energy, average velocity, and frequency of collisions of gas molecules with the walls of the container increase, decrease, or remain the same under each of the following conditions? a. The temperature is increased to 260°C. Average kinetic energy Average velocity The collision frequency b. The temperature is decreased to -40°C. Average kinetic energy Average velocity The collision frequency c. The volume is decreased to 0.2 L. Average kinetic energy Average velocity The collision frequency d. The number of moles of neon is doubled. Average kinetic energy Average velocity The collision frequency

Consider a 1.0-L container of neon gas at STP. Will the average kinetic energy, average velocity, and frequency of collisions of gas molecules with the walls of the container increase, decrease, or remain the same under each of the following conditions? a. The temperature is increased to 220°C. Average kinetic energy Average velocity The collision frequency The temperature is decreased to -70°C. Average kinetic energy Average velocity The collision frequency c. The volume is decreased to 0.3 L. Average kinetic energy Average velocity The collision frequency d. The number of moles of neon is tripled. Average kinetic energy Average velocity The collision frequency Visited ↑ ↑ ↑ ↑ ♥ ♥ ↑ ↑ ↑ ↑ ↑ ↑