Chemistry - Thermochemistry Question with Solution | TestHub

ChemistryThermochemistryEnthalpy of ReactionEasy2 minPYQ_2020

ChemistryEasysingle choice

If $∆ H_{f}^{o}$ for $H_{2} O_{2}$ and $H_{2} O$ are -188 kJ/mol and -286 kJ/mol, what will be the enthalpy change of the reaction:

$2 H_{2} O_{2} (l) \to 2 H_{2} O (l) + O_{2} (g)$

Options:

Answer:

Solution:

Given reaction is $2 H_{2} O_{2} (l) \to 2 H_{2} O (l) + O_{2} (g)$

${ΔH}_{Reaction}^{o} = {ΔH}_{f}^{o} (Products) - {ΔH}_{f}^{o} (Reactants)$

Enthalpy change $= 2 \times (- 286) - (2 \times - 188)$

$= - 196 k J$

Stream:NTA_ABHYAS_NEETSubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of Reaction

⏱ 2mℹ️ Source: PYQ_2020

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