(C) The reaction is $C_2H_2 + H_2 \rightarrow C_2H_4$. We use the formula: $\Delta H_{reaction} = \sum \Delta H_{comb}^o (Reactants) - \sum \Delta H_{

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(C) The reaction is $C_2H_2 + H_2 \rightarrow C_2H_4$. We use the formula: $\Delta H_{reaction} = \sum \Delta H_{comb}^o (Reactants) - \sum \Delta H_{comb}^o (Products)$. Given: $\Delta H_{comb}^o (C_2H_2) = -337.2 \ K \ cal \ mol^{-1}$ $\Delta H_{comb}^o (H_2) = \Delta H_f^o (H_2O) = -68.3 \ K \ cal \ mol^{-1}$ $\Delta H_{comb}^o (C_2H_4) = -363.7 \ K \ cal \ mol^{-1}$ Substituting the values: $\Delta H = [(-337.2) + (-68.3)] - (-363.7)$ $\Delta H = -405.5 + 363.7 = -41.8 \ K \ cal$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

The heat of reaction for $C_2H_2 + H_2 \rightarrow C_2H_4$ is given by the following data:
$(i) \Delta H_f^o \text{ of } H_2O_{(\ell)} = -68.3 \ K \ cal \ mol^{-1}$
$(ii) \Delta H_{comb}^o \text{ of } C_2H_2 = -337.2 \ K \ cal \ mol^{-1}$
$(iii) \Delta H_{comb}^o \text{ of } C_2H_4 = -363.7 \ K \ cal \ mol^{-1}$

A
$-716.1$
B
$+337.2$
C
$-41.8$
D
$-579.5$

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Mix Examples-Thermodynamics and Thermochemistry

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Observe the following reactions: $AB_{(g)} + 25 H_2O_{(l)} \rightarrow AB_{(25 H_2O)} ; \Delta H = x \ kJ \ mol^{-1}$ $AB_{(g)} + 50 H_2O_{(l)} \rightarrow AB_{(50 H_2O)} ; \Delta H = y \ kJ \ mol^{-1}$ The enthalpy of dilution $(\Delta H_{dil})$ in $kJ \ mol^{-1}$ is

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Observe the following reactions:
$AB_{(g)} + 25 H_2O_{(l)} \rightarrow AB_{(25 H_2O)} ; \Delta H = x \ kJ \ mol^{-1}$
$AB_{(g)} + 50 H_2O_{(l)} \rightarrow AB_{(50 H_2O)} ; \Delta H = y \ kJ \ mol^{-1}$
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