Question #0e77c
1 Answer
Nov 11, 2017
Pressure IS affected by temperature.
Under the condition that no environmental variable is held constant in a closed system (thus, the mols are held constant),
#P_1V_1 = nRT_1#
#P_2V_2 = nRT_2#
for an ideal gas. And so,
#(P_1V_1)/T_1 = (P_2V_2)/T_2 = nR#
Therefore, if you increase the pressure, you increase the temperature and vice versa.
- Higher temperatures increase collisions with the wall, thus increasing the pressure of the gas onto the wall.
- Higher gas pressures are due to greater collisions on the walls, which increases the average kinetic energy. Therefore, since the average kinetic energy is proportional to the temperature, the temperature increases due to an increase in pressure.
