Given the following thermochemical data:

$C_2{H}_{2(g)}+\frac{5}{2}{O}_{2()}2C{O}_{2(g)}+H_2{O}_{(0)}H=-1\mathrm{.}30{10}^{3}kJ$

$C_2{H}_{6(g)}+\frac{7}{2}{O}_{2()}2C{O}_{2()}+3H_2{O}_{(i)}H=-1\mathrm{.}56{10}^{3}kJ$

$H_{2()}+\frac{1}{2}{O}_{2(0)}{H}_2{O}_{(0)}H=-2\mathrm{.}86{10}^{2}kJ$

What is $H$ for the following reaction?

$C_2{H}_{2(g)}+2H_{2(g)}{C}_2{H}_{6(g)}$

a$.-2\mathrm{.}60{10}^{1}kJ$

d$.-5\mathrm{.}46{10}^{3}kJ$

b$.-3\mathrm{.}12{10}^{2}kJ$

e$.2\mathrm{.}60{10}^{1}kJ$

c$.-5\mathrm{.}72{10}^{2}kJ$