Question

Suppose a sample of an ideal gas in a container is subjected to a temperature change. A decrease in temperature will the kinetic energy and average speed of the gas particles. As a result, the pressure on the walls of the container will If the gas starts at 25 ∘ C, what temperature would the gas need to reach for its pressure to double? temperature = ∘ C

Answer 1

Decrease, decrease, 323 °C

Step-by-step explanation:

Suppose a sample of an ideal gas in a container is subjected to a temperature change. A decrease in temperature will decrease the kinetic energy and average speed of the gas particles. As a result, the pressure on the walls of the container will decrease. If the gas starts at 25 °C, what temperature would the gas need to reach for its pressure to double?

The initial temperature is 25°C + 273 = 298 K. We want the pressure P₂ to be the double of the pressure P₁. We can find the required temperature T₂ using Gay-Lussac's law.

`(P_(1))/(T_(1)) =(P_(2))/(T_(2)) \\(P_(1))/(T_(1)) =(2P_(1))/(T_(2))\\T_(2)=2T_(1)=2 * 298K =596 K`

T₂ = 596 K - 273 = 323 °C