Chemistry - Thermochemistry Question with Solution | TestHub

When $400 \mathrm{mL}$ of $0.2 \mathrm{M} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution is mixed with $600 \mathrm{mL}$ of $0.1\mathrm{MNaOH}$ solution, the increase in temperature of the final solution is $—\times {10}^{-2} \mathrm{K}$. (Round off to the nearest integer).

[Use :${\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)\to {\mathrm{H}}_2\mathrm{O}:$$\left.{\Delta }_{\gamma }\mathrm{H}=-57.1 \mathrm{kJ}{ \mathrm{mol}}^{-1}\right]$ 

Specific heat of ${\mathrm{H}}_2\mathrm{O}=4.18 \mathrm{J}{ \mathrm{K}}^{-1}{ \mathrm{g}}^{-1}$ , density of ${\mathrm{H}}_2\mathrm{O}=1.0 \mathrm{g}{ \mathrm{cm}}^{-3}$ 

Assume no change in volume of solution on mixing.