For the reactions,$C + O_2 \to CO_2; \Delta H = -393 \ J$
$2Zn + O_2 \to 2ZnO; \Delta H = -412 \ J$

Calculate the enthalpy change when $6 \text{ g}$ of $CO(g)$ reacts with sufficient $NO_2(g)$ according to the following reaction: $4 \text{ CO}(g) + 2 \text{ NO}_2(g) \rightarrow 4 \text{ CO}_2(g) + 2 \text{ N}_2(g)$; $\Delta_r H^0 = -1200 \text{ kJ}$ (in $\text{ kJ}$)

The $\Delta E^o$ of combustion of $2-$methylpropene is $-X \ kJ \ mol^{-1}$. The value of $\Delta H^o$ is

For the reaction: $A_{(g)} + B_{(s)} \rightleftharpoons 2C_{(g)} + D_{(g)}$,given $\Delta U = 5.0 \ kcal$ and $\Delta S = 50 \ cal \ K^{-1}$ at $400 \ K$. Calculate $\Delta G$ for the reaction. (in $kcal$)

Given below are two statements:
Statement-$I$: For isothermal irreversible change of an ideal gas,$q = -w = P_{\text{ext}} (V_{\text{final}} - V_{\text{initial}})$
Statement-$II$: For adiabatic change,$\Delta U = W_{\text{adiabatic}}$
The correct answer is

Which of the following relations is not correct?