When 400 {mL} of 0.2 {M} {H}_{2} {SO}_{4} solution is mixed with 600 {mL} of 0.1 {M} {NaOH} solution, the increase in temperature of the final solution is -10^{-2} {K}. (Round off to the nearest integer). [Use : {H}^{+}({aq})+{OH}^{-}({aq}) \\to {H}_{2} {O}: \\Delta_{\\gamma} {H}=-57.1 {kJ} {mol}^{-1}] Specific heat of {H}_{2} {O}=4.18 {J} {K}^{-1} {g}^{-1} density of {H}_{2} {O}=1.0 {g} {cm}^{-3} Assume no change in volume of solution on mixing. [27 Jul 2021 Shift 2]

JEE Main 27 July 2021 Shift 2 Solved Paper

Section: Chemistry

Question : 52 of 90

Marks: +1, -0

When 400mL of 0.2MH2SO4 solution is mixed with 600mL of 0.1MNaOH solution, the increase in temperature of the final solution is −10−2K. (Round off to the nearest integer).
[Use : H+(aq)+OH−(aq)→H2O:
ΔγH=−57.1kJmol−1]
Specific heat of H2O=4.18JK−1g−1
density of H2O=1.0gcm−3
Assume no change in volume of solution on mixing.

[27 Jul 2021 Shift 2]

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