MCQ
The enthalpy change $(\Delta H)$ for the reaction, $N_2(g) + 3H_2(g) \to 2NH_3(g)$ is $-92.38\, KJ$ at $298\, K$ . The internal energy change $\Delta U$ at $298\, K$ is ....$ KJ$
- A$-92.38$
- ✓$-87.42$
- C$-97.34$
- D$-89.9$
$\Delta H=-92.38 kJ$ at $298 K$
$\Delta E=?$
$\Delta H=\Delta E+\Delta n R T$
$\Delta n=2-(3+1)$
$=-2-92.38 \times 10^{3}$
$=\Delta E+8.314 \times(-2) \times 298$
$\Delta E=-87424.8 J =-87.425 kJ$
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$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$
has a value of $278$ at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature?
$SO_{3(g)} \rightleftharpoons SO_{2(g)} + \frac{1}{2} O_{2(g)}$
$\mathop {Al}\limits_{metal} \xrightarrow[{(aq.)}]{{HCl}}'X' + Gas\,'P'$
$\mathop {Al}\limits_{metal} \xrightarrow[{ + {H_2}O}]{{NaOH\,(aq.)}}'Y' + Gas\,'Q'$
$(R = 8.314\,J\,{\rm{degre}}{{\rm{e}}^{{\rm{ - 1}}}}mo{l^{ - 1}})$