Class 11 Chemistry | Thermodynamics | State Board | Mixed Level Practice Test (2026)

Which of the following is an example of an extensive property?

The first law of thermodynamics is based on the conservation of:

For an endothermic reaction, which of the following statements is true?

What is the change in internal energy ($\Delta U$) if 100 J of heat is added to the system and 50 J of work is done by the system?

Which of the following conditions would always lead to a spontaneous reaction?

The standard enthalpy of formation is zero for which of the following substances in their standard states?

Which of the following processes results in an increase in entropy?

Calculate the work done in an isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 L to 20 L at 300 K. (R = 8.314 J/mol.K)

What is the relationship between Gibbs free energy change ($\Delta G$), enthalpy change ($\Delta H$), and entropy change ($\Delta S$) at constant temperature ($T$)?

For a reaction to be non-spontaneous at all temperatures, which of the following conditions must be true?

Which of the following is an intensive property?

For an ideal gas, the change in internal energy ($\Delta U$) is always zero for which type of process?

What is the relationship between enthalpy change ($\Delta H$) and internal energy change ($\Delta U$) for a reaction involving gases, where $\Delta n_g$ is the change in the number of moles of gaseous reactants and products?

Which of the following statements is true for a spontaneous process?

The heat of combustion of methane, $CH_4(g)$, is $-890 kJ/mol$. What is the value of $\Delta U$ when 1 mole of $CH_4(g)$ is completely combusted at 298 K?

What is the standard enthalpy of formation ($\Delta H_f^\circ$) of an element in its standard state?

A system absorbs 600 J of heat and does 200 J of work. What is the change in internal energy ($\Delta U$) for the system?

Which of the following conditions would favor the spontaneity of a reaction where both enthalpy change ($\Delta H$) and entropy change ($\Delta S$) are positive?

For the reaction $N_2(g) + 3H_2(g) ightleftharpoons 2NH_3(g)$, $\Delta H = -92.2 kJ$. What is the value of $\Delta H$ if the reaction is written as $2NH_3(g) ightleftharpoons N_2(g) + 3H_2(g)$?

Calculate the entropy change ($\Delta S$) when 1 mole of an ideal gas expands isothermally and reversibly from a volume of $10 L$ to $100 L$ at $300 K$.

Which of the following statements is correct regarding the first law of thermodynamics?

What is the change in internal energy ($\Delta U$) if a system absorbs 300 J of heat and does 500 J of work?

Which of the following processes is adiabatic?

What is the enthalpy change ($\Delta H$) for a reaction if the internal energy change ($\Delta U$) is -100 kJ and the work done ($P\Delta V$) is 10 kJ?

Which of the following is a state function?

Calculate the standard enthalpy change ($\Delta H^\circ$) for the reaction: $N_2(g) + 3H_2(g) ightarrow 2NH_3(g)$, given that the standard enthalpy of formation of $NH_3(g)$ is -46 kJ/mol.

What is the entropy change ($\Delta S$) for a reversible process at constant temperature (T) when the heat absorbed is q?

For a spontaneous process, which of the following conditions must be true?

If the equilibrium constant for a reaction is $K = 1$, what is the value of $\Delta G^\circ$?

Which of the following reactions is most likely to have a positive entropy change ($\Delta S > 0$)?

Which of the following is an example of an intensive property?

For an adiabatic process, which of the following is true?

The enthalpy change for a reaction is $-50$ kJ/mol. What can be inferred about the reaction?

What is the standard enthalpy of formation of an element in its standard state?

Which of the following conditions favors the spontaneity of a reaction according to Gibbs free energy equation, $\\Delta G = \\Delta H - T\\Delta S$?