NEET Chemistry: Thermodynamics — Practice Set 6

Q1. The work done in the reversible adiabatic expansion of 1 mol of an ideal gas from 10 L to 20 L is (\( \gamma = 1.4 \)) at 300 K. Calculate \( w \). (\( R = 8.314 \, \text{J/mol·K} \))

Q2. Which of the following is always true for a spontaneous process at constant temperature and pressure?

Q3. Calculate \(\Delta S_{surr}\) when 2 mol of a substance melts at 300 K if \(\Delta H_{fus} = 8 \, \text{kJ/mol}\).

Q4. A reaction has \( \Delta H = 80.00 \, \text{kJ/mol} \), \( \Delta S = 200.0 \, \text{J/K·mol} \), and is spontaneous at 450 K. What is \( \Delta G \) at 450 K?

Q5. Calculate \(\Delta H\) for the reaction \(C(s) + 2H_2(g) \rightarrow CH_4(g)\) given: \(CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(l)\), \(\Delta H = -890.3 \, \text{kJ/mol}\); \(C(s) + O_2(g) \rightarrow CO_2(g)\), \(\Delta H = -393.5 \, \text{kJ/mol}\); \(H_2(g) + \frac{1}{2}O_2(g) \rightarrow H_2O(l)\), \(\Delta H = -285.8 \, \text{kJ/mol}\).

Q6. For the process \(H_2O(l) \rightarrow H_2O(g)\) at 373 K, \(\Delta H = 40.79 \, \text{kJ/mol}\), what is \(\Delta S_{surr}\)?

Q7. The standard enthalpy of formation of \(NH_3(g)\) is -46.1 kJ/mol. What is \(\Delta H\) for \(N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)\)?

Q8. For an ideal gas expanding reversibly and adiabatically, the relationship between temperature and volume is:

Q9. For the reaction \( 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \), \( \Delta H = -483.6 \, \text{kJ/mol} \) at 298 K. What is \( \Delta U \)? (\( R = 8.314 \, \text{J/mol·K} \))

Q10. A reaction has \(\Delta H = -100 \, \text{kJ}\) and \(\Delta S = -200 \, \text{J/K}\). At what temperature does it become spontaneous?

Chemistry — Thermodynamics

Set 6 of 20

15:00

Sign in to save your score and view detailed explanations

Sign In Free
1Question 1 of 10
Medium

The work done in the reversible adiabatic expansion of 1 mol of an ideal gas from 10 L to 20 L is (\( \gamma = 1.4 \)) at 300 K. Calculate \( w \). (\( R = 8.314 \, \text{J/mol·K} \))