Thermodynamics — MCQ Practice

Which of the following statements is INCORRECT regarding a spontaneous process?

Calculate the work done during the expansion of a gas from $4,\text{L}$ to $6,\text{L}$ against a constant external pressure of $2.5,\text{atm}$.

For the reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$, if $\Delta H = -92.4,\text{kJ}$ at $298,\text{K}$, what is the value of $\Delta U$ for the reaction? (Given $R = 8.314,\text{J/mol K}$)

Which of the following processes leads to an increase in entropy?

For a certain reaction, $\Delta H = -200,\text{kJ}$ and $\Delta S = -50,\text{J/K}$. At what temperature will the reaction become spontaneous?

An ideal gas expands reversibly and isothermally from an initial volume of $10,\text{L}$ to a final volume of $20,\text{L}$ at $300,\text{K}$. If $2,\text{moles}$ of the gas are used, calculate the work done. (Given $R = 8.314,\text{J/mol K}$)

Which of the following statements is true for an adiabatic process?