200 mL of 0.2 M HCl is mixed with 300 mL of 0.1 M NaOH. The molar heat of neutralization of this reaction is -57.1 kJ. The increase in temperature in…

$\displaystyle 200$ mL of $\displaystyle 0.2$ M HCl is mixed with $\displaystyle 300$ mL of $\displaystyle 0.1$ M NaOH . The molar heat of neutralization of this reaction is -$\displaystyle 57.1$ kJ. The increase in temperature in °C of the system on mixing is $\displaystyle x \times 10^{-2}$. The value of $\displaystyle x$ is \_\_\_\_. (Nearest integer) [Given : Specific heat of water $\displaystyle =4.18 \mathrm{~J} \mathrm{~g}^{-1} \mathrm{~K}^{-1}$ Density of water $\displaystyle =1.00 \mathrm{~g} \mathrm{~cm}^{-3}$ ] (Assume no volume change on mixing)