Calculate \Delta {\kern 1pt} H_{{\rm{rxn}}} for the following reaction:

Calculate Delta {kern 1pt} H_{{rm{rxn}}} for the following reaction:{rm{CH}}_4 (g); + ;4{rm{ Cl}}_2 (g); rightarrow ;{rm{CCl}}_4 (g); + ;4{rm{ HCl(}}g)Use the following reactions and given Delta H{rm{'s}}.begin{array}{c} {rm{C(}}s); + ;2{rm{ H}}_2 (g); rightarrow ;{rm{CH}}_4 (g){rm{ }};;Delta H = - 74.6;{rm{ kJ}} \ {rm{C(}}s); + ;2;{rm{Cl}}_2 (g); rightarrow ;{rm{CCl}}_4 (g){rm{ }};;Delta H = - 95.7;{rm{ kJ}} \ {rm{H}}_2 (g); + ;{rm{Cl}}_2 (g); rightarrow ;2{rm{ HCl(}}g){rm{ }};;Delta H = - 184.6;{rm{ kJ}} \ end{array}