Question

A gas is heated from 263.0 K to 298.0 K and the volume is increased from 24.0 liters to 35.0 liters by moving a large piston within a cylinder. If the original pressure was 1.00 atm, what would the final pressure be?

Answer 1

The final pressure is approximately 0.78 atm

Step-by-step explanation:

The original temperature of the gas, T₁ = 263.0 K

The final temperature of the gas, T₂ = 298.0 K

The original volume of the gas, V₁ = 24.0 liters

The final volume of the gas, V₂ = 35.0 liters

The original pressure of the gas, P₁ = 1.00 atm

Let P₂ represent the final pressure, we get;

`(P_1 \cdot V_1)/(T_1) = (P_2 \cdot V_2)/(T_2)`

`P_2 = (P_1 \cdot V_1 \cdot T_2)/(T_1 \cdot V_2)`

`P_2 = (1 * 24.0 * 298)/(263.0 * 35.0) = 0.776969038566`

∴ The final pressure P₂ ≈ 0.78 atm.