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ChemistryThermochemistryHess's Law of Constant Heat SummationMedium2 minQB

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$H^{+} + OH^{-} ⟶ H_{2} O; Δ H^{\circ} = - 57 kJ / mol$

$Δ H_{i o ni s a t i o n}^{\circ}$ $[HCN] = 45 kJ/mol$

If $200 mL$ of $1/10 M$ $Ba (OH)_{2}$ solution is mixed with $500 mL$ of $1/10 M$ $HCN$ , then the evolved heat will be:

Answer:

Solution:

L.R.

Ba(OH)₂ + 2HCN → Ba(CN)₂ + 2H₂O

20 50 $Δ H = - 24 k J / m o l$

millimol millimol

Heat evolved will be:

$24 k J / m o l \times 20 mm o l = 24 \times 20 \times 1 0^{- 3} k J = 480 \times 1 0^{- 3} k J = 0.48 k J = 480 J$

Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Hess's Law of Constant Heat Summation

⏱ 2mℹ️ Source: QB

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