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

Answer:

Decrease, decrease, 323 °C

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.

$\frac{P_{1}}{T_{1}} =\frac{P_{2}}{T_{2}} \\\frac{P_{1}}{T_{1}} =\frac{2P_{1}}{T_{2}}\\T_{2}=2T_{1}=2 \times 298K =596 K$

T₂ = 596 K - 273 = 323 °C