1 mole of $H_{2} S O_{4}$ is mixed with excess of NaOH in a dilute solution. The enthalpy change is nearly equal to

57.3 kJ

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114.6 kJ

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-114.6 kJ

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-57.3 kJ

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Solution

The correct option is C
-114.6 kJ

1 mole of $H_{2} S O_{4} \equiv 2 e q u i v .$

$Δ H_{N} = 2 \times (- 57.3) = - 114.6 k J$

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1 mole of H2SO4 is mixed with excess of NaOH in a dilute solution. The enthalpy change is nearly equal to

The correct option is C -114.6 kJ 1 mole of H2SO4≡2 equiv. ΔHN=2×(−57.3)=−114.6 kJ

1 mole of $H_{2} S O_{4}$ is mixed with excess of NaOH in a dilute solution. The enthalpy change is nearly equal to

The correct option is C
-114.6 kJ

1 mole of $H_{2} S O_{4} \equiv 2 e q u i v .$

$Δ H_{N} = 2 \times (- 57.3) = - 114.6 k J$