7 questions · self-marked practice — reveal the answer and mark yourself.
| Column A | Column B |
| (1) Isochoric process | (a) zero |
| (2) First law of thermodynamics | (b) $d V=0$ |
| (3) Density | (c) $\Delta U = q + w$ |
| (4) Enthalpy of formation of any element in transition state | (d) intensive property |
| Column A | Column B |
| (1) $\Delta H _s$ | (a) R |
| (2) $C _{ p }- C _{ V }$ | (b) System + surroundings |
| (3) Law of conservation of energy | (c) $\Delta H _{ f }+\Delta H _V$ |
| (4) Universe | (d) First law of thermodynamics |
| Column A | Column B |
| (1) Neutralization energy of HCl + NaOH | (a) Heat exchange due to difference in temperature |
| (2) Formation of mixture of gases | (b) 57.32 kJ |
| (3)$\Delta G$ > 0 | (c) increase in entropy |
| (4) Heat | (d) non-spontaneous process |
| Column A | Column B |
| (1) Enthalpy of solution | (a) irreversible process |
| (2) Volume | (b) decrease in entropy |
| (3) Spontaneous process | (c) hydration enthalpy/ salvation enthalpy |
| (4) Crystallisation of sugar from solution | (d) Extensive property |
| Column A | Column B |
| (1) For isothermal reversible process | (a) calculation of combustion energy |
| (2) Entropy change at equilibrium | (b) $\begin{array}{l} W _{ rev }=-2303 nRT \\ \log \frac{ V _{ f }}{ V _{ i }}\end{array}$ |
| (3) Ideal process | (c) $\Delta S =0$ |
| (4) Bomb calorimeter | (d) reversible process |
| Column A | Column B |
| (1) Spontaneous process | (a) conversion of ice to water |
| (2) Entropy | (b) $\Delta G$ negative |
| (3) Mechanical energy | (c) Measure of disorder of system |
| (4) Isothermal process | (d) conversion of mechanical energy to kinetic energy |
| Column A | Column B |
| (1) Standard state of substance | (a) $\Delta G =\Delta H - T \Delta S$ |
| (2) Entropy of sublimation | (b) 1 atm pressure and 298 K temperature |
| (3) Gibbs equation | (c) non-crystalline |
| (4) Glass | (d) $\Delta S _{\text {sub }}=\frac{\Delta H _{\text {(sub) }}}{ T }$ |