The amount of energy released when $$20\,mL$$ of $$0.5\,M\,NaOH$$ are mixed with $$100\,mL$$ of $$0.1\,M\,HCl$$ is $$x\,kJ.$$ The heat of neutralisation $$\left( {{\text{in}}\,\,kJ\,mo{l^{ - 1}}} \right)$$ is
A.
$$- 100\,x$$
B.
$$- 50\,x$$
C.
$$+ 100\,x$$
D.
$$+ 50\,x$$
Answer :
$$- 100\,x$$
Solution :
In question $$0.01\,gev$$ of $$NaOH$$ is being neutralised by $$0.01\,gev$$ of $$HCl$$ and value is $$x\,kJ,$$ for $$1\,gev$$ the value is $$ - 100x$$ ( exothermic process ).
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 $$C{O_2}\left( g \right) + {H_2}\left( g \right) \to CO\left( g \right) + {H_2}O\left( g \right)\,{\text{is}}$$