A cylinder of gas at a temperature of 21^oC has a pressure of 3.8 atm. If the closed cylinder were heated in a fire to a temperature of 365^oC, what would be the new pressure?

Question

Quizplus · Accepted Answer

To find the new pressure, use the ideal gas law in the form of $P_1/T_1 = P_2/T_2$, where temperatures must be in Kelvin. Convert temperatures from Celsius to Kelvin by adding 273.15. Thus, $T_1 = 294.15K$ and $T_2 = 638.15K$. Solving for $P_2$, $P_2 = P_1 \times (T_2/T_1) = 3.8 \times (638.15/294.15) \approx 8.2 atm$.

A Cylinder of Gas at a Temperature of 21oC Has

A Cylinder of Gas at a Temperature of 21^oC Has