Exams › JEE Main › Chemistry
500 J of energy is transferred as heat to 0.5 mol of Argon gas at 298 K and 1.00 atm. The final temperature and the change in internal energy respectively are : Given : R = 8.3 J K^-1 mol^-1
- (1) 348 K and 300 J
- (2) 378 K and 300 J
- (3) 368 K and 500 J
- (4) 378 K and 500 J
Correct answer: (1) 348 K and 300 J
Solution
The correct option is right because the heat transferred to the gas increases its temperature, calculated using the ideal gas equation and the specific heat capacity for a monatomic gas like Argon. The change in internal energy is also consistent with the first law of thermodynamics, which accounts for the heat added and the work done on the system.
Related JEE Main Chemistry questions
- Using the following thermochemical equations, determine the enthalpy of vaporisation of water: \[ \mathrm{H_2(g) + \tfrac{1}{2}O_2(g) \to H_2O(l)},\quad \Delta H = -286\ \text{kJ} \] \[ \mathrm{H_2(g) + \tfrac{1}{2}O_2(g) \to H_2O(g)},\quad \Delta H = -245.5\ \text{kJ} \]
- Given that the standard enthalpy of formation of NH$_3$ is $-46.0\ \text{kJ mol}^{-1}$, and the enthalpy of formation of H$_2$ from gaseous atoms is $-436\ \text{kJ mol}^{-1}$ while that of N$_2$ from gaseous atoms is $-712\ \text{kJ mol}^{-1}$, what is the average N–H bond enthalpy in NH$_3$?
- Using the following bond dissociation data, determine the enthalpy change for the conversion $8S(s) + \tfrac32 S_8(g)$.
- Using the bond enthalpies given below, determine the enthalpy change for the hydrogenation reaction shown: H–H bond energy = 431.37 kJ mol$^{-1}$ C–C bond energy = 606.10 kJ mol$^{-1}$ C–H bond energy = 336.49 kJ mol$^{-1}$ C–H bond energy = 410.50 kJ mol$^{-1}$ $C=C + H–H \rightarrow H–C–C–H$ What is the enthalpy change for this reaction?
- For a given reversible reaction, both enthalpy change ($\Delta H$) and entropy change ($\Delta S$) are positive. If $T_1$ denotes the equilibrium temperature, under which condition will the reaction be spontaneous?
- For the spontaneous reaction $2C_2H_6(g) + 25O_2(g) \rightarrow 16CO_2(g) + 18H_2O(g)$, what are the signs of $\Delta H$, $\Delta S$, and $\Delta G$ in that order?
⚔️ Practice JEE Main Chemistry free + battle 1v1 →