Chemistry

Chemistry

Problem

Given that | C2H6(g)+Cl2(g)→ΔH1=−99 kJ mol−1\text{C}_2\text{H}_6(\text{g}) + \text{Cl}_2(\text{g}) \rightarrow \quad \Delta H_1 = -99 \text{ kJ mol}^{-1} | |---| | C2H5Cl(g)+HCl(g)\text{C}_2\text{H}_5\text{Cl}(\text{g}) + \text{HCl}(\text{g}) | | H2(g)+Cl2(g)→ΔH2=−185 kJ mol−1\text{H}_2(\text{g}) + \text{Cl}_2(\text{g}) \rightarrow \quad \Delta H_2 = -185 \text{ kJ mol}^{-1} | |---| | 2HCl(g)2\text{HCl}(\text{g}) | | C2H4(g)+H2(g)→ΔH3=−136 kJ mol−1\text{C}_2\text{H}_4(\text{g}) + \text{H}_2(\text{g}) \rightarrow \quad \Delta H_3 = -136 \text{ kJ mol}^{-1} | |---| | C2H6(g)\text{C}_2\text{H}_6(\text{g}) | calculate the enthalpy change for the following reaction: C2H4+HCl→C2H5Cl\text{C}_2\text{H}_4 + \text{HCl} \rightarrow \text{C}_2\text{H}_5\text{Cl}

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