Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 $$K.$$ The enthalpy change ( in $$kJ$$ ) for the process is
A.
$$11.4 kJ$$
B.
$$-11.4 kJ$$
C.
$$0 kJ$$
D.
$$4.8 kJ$$
Answer :
$$0 kJ$$
Solution :
$$\Delta H = n{C_p}\,\Delta T$$ solution; since $$\Delta T = 0\,{\text{so}},\,\,\Delta H = 0$$
Releted MCQ Question on Physical Chemistry >> Chemical Thermodynamics
Releted Question 1
The difference between heats of reaction at constant pressure and constant volume for the reaction : $$2{C_6}{H_6}\left( l \right) + 15{O_{2\left( g \right)}} \to $$ $$12C{O_2}\left( g \right) + 6{H_2}O\left( l \right)$$ at $${25^ \circ }C$$ in $$kJ$$ is
$${\text{The}}\,\Delta H_f^0\,{\text{for}}\,C{O_2}\left( g \right),\,CO\left( g \right)\,$$ and $${H_2}O\left( g \right)$$ are $$-393.5,$$ $$-110.5$$ and $$ - 241.8\,kJ\,mo{l^{ - 1}}$$ respectively. The standard enthalpy change ( in $$kJ$$ ) for the reaction $$C{O_2}\left( g \right) + {H_2}\left( g \right) \to CO\left( g \right) + {H_2}O\left( g \right)\,{\text{is}}$$