200 joules of heat was supplied to a system at constant volume. It resulted in the increase in temperature of the system from 298 to 323$$\,K.$$ What is the change in internal energy of the system ?
A.
400$$\,J$$
B.
200$$\,J$$
C.
50$$\,J$$
D.
150$$\,J$$
Answer :
200$$\,J$$
Solution :
$$\eqalign{
& {\text{At constant volume,}}\,\Delta V = 0 \cr
& w = - P\Delta V = 0\,\,\,\,\,\Delta U = q = 200\,J \cr} $$
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 $$C{O_2}\left( g \right) + {H_2}\left( g \right) \to CO\left( g \right) + {H_2}O\left( g \right)\,{\text{is}}$$