A mixture of two moles of carbon monoxide and one mole of oxygen, in a closed vessel is ignited to convert the carbon monoxide to carbon dioxide. If $$\Delta H$$ is the enthalpy change and $$\Delta E$$ is the change in internal energy, then
The value of enthalpy change $$(\Delta H)$$ for the reaction $$\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}(l)+3 \mathrm{O}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{CO}_2(\mathrm{~g})+ 3 \mathrm{H}_2 \mathrm{O}(l)$$, at $$27^{\circ} \mathrm{C}$$ is $$-1366 \cdot 5 \mathrm{~kJ} \mathrm{~mol}^{-1}$$. The value of internal energy change for the above reaction at this temperature will be
Standard entropy of X2, Y2 and XY3 are 60, 40 and 50 JK$$-$$1mol$$-$$1, respectively. For the reaction, $$\frac{1}{2}$$X2 + $$\frac{3}{2}$$Y2 $$\to$$ XY3, $$\Delta$$H = $$-$$30 kJ, to be at equilibrium, the temperature will be
In an adiabatic process, no transfer of heat takes place between system and surrounding. Choose the correct option for free expansion of an ideal gas under adiabatic condition from the following.