A cylinder containing 5.00 mol of nitrogen gas is at room temperature (300 K).If the pressure of the gas is held constant and the gas is heated,how much energy must be transferred by heat to the gas to increase its temperature by 100 K?

Question

Quizplus · Accepted Answer

The energy transferred by heat can be calculated using the formula $q = nC_{p}\Delta T$, where $n$ is the number of moles, $C_{p}$ is the molar heat capacity at constant pressure, and $\Delta T$ is the change in temperature. For nitrogen gas ($N_2$), $C_{p}$ is approximately 29.1 J/mol·K. Thus, $q = 5.00 \, \text{mol} \times 29.1 \, \text{J/mol·K} \times 100 \, \text{K} = 1.455 \times 10^4 \, \text{J}$, which rounds to 1.46 x $10^4$ J.

A Cylinder Containing 5