The constant pressure molar heat capacity of methane, CH₄, is 35.31 J K^-1 mol^-1 at temperatures close to 298 K. Calculate the enthalpy change when 2.00 mol of methane is heated from a temperature of 278 K to 318 K.

Question

Quizplus · Accepted Answer

The enthalpy change ($\Delta H$) can be calculated using the formula $\Delta H = nC_p\Delta T$, 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. Plugging in the given values: $\Delta H = 2.00 \, \text{mol} \times 35.31 \, \text{J K}^{-1} \text{mol}^{-1} \times (318 \, \text{K} - 278 \, \text{K}) = 2.83 \, \text{kJ}$.

The Constant Pressure Molar Heat Capacity of Methane, CH4, Is

The Constant Pressure Molar Heat Capacity of Methane, CH₄, Is