When 400 mL of 0.2 M H₂SO₄ 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) → H₂O: Δ _ γ H = - 57.1 kJ mol⁻¹] Specific heat of H₂O = 4.18 J K⁻¹ g⁻¹ density of H₂O = 1.0 g cm⁻³ Assume no change in volume of solution on mixing.

Chemical Thermodynamics: JEE Main 2021 Chemistry question

JEE Main 2021 · 27 Jul, Evening shift · Q24

JEE Main 202127 Jul, Evening shiftChemistryHardChemical Thermodynamics84× since 2002

When 400 mL of 0.2 M H₂SO₄ solution is mixed with 600 mL of 0.1 M NaOH solution, the increase in temperature of the final solution is __________

\times

10^

-

2 K. (Round off to the nearest integer). [Use : H⁺ (aq) + OH^

-

(aq)

\to

H₂O :

\Delta

\gamma

H =

-

57.1 kJ mol^

-

1] Specific heat of H₂O = 4.18 J K^

-

1 g^

-

1 density of H₂O = 1.0 g cm^

-

3 Assume no change in volume of solution on mixing.

Your answerType your answer. Integers and decimals are accepted.

JEE Main 2021 Chemical Thermodynamics Question with Answer (27 Jul Evening shift, Q24) | JEE Arc