Question

1. what effect does raising the temperature of a gas have on its pressure, if the volume of the gas and the number of its particles are kept constant?
2. how does reducing the volume of a gas affect its pressure if the temperature of the gas and the number of particles are constant?

Explanation:

Question 6

To determine the effect of raising the temperature of a gas on its pressure (with volume and number of particles constant), we use the ideal gas law ($PV = nRT$) or the kinetic theory of gases. When temperature ($T$) increases, gas particles gain kinetic energy, move faster, and collide with the container walls more frequently and forcefully. Since volume ($V$) and moles ($n$) are constant, pressure ($P$) must increase to balance the equation $PV = nRT$ (as $T \uparrow$, $P \uparrow$ to maintain equality).

To determine the effect of reducing the volume of a gas on its pressure (with temperature and number of particles constant), we use the ideal gas law ($PV = nRT$) or the kinetic theory of gases. When volume ($V$) decreases, gas particles have less space to move, so they collide with the container walls more frequently. Since temperature ($T$) and moles ($n$) are constant, pressure ($P$) must increase to balance the equation $PV = nRT$ (as $V \downarrow$, $P \uparrow$ to maintain equality).

Answer:

Raising the temperature of a gas (with constant volume and number of particles) increases its pressure. This is because higher temperature increases particle kinetic energy, leading to more frequent and forceful collisions with the container, which raises pressure.

Question 7