At 1000k delta h 12377 kjmol for the reaction n2g h2g 2nh3g...

At 1000.K, delta H=-123.77 Kj/mol for the reaction N2(g) + #H2(g) -> 2NH3(g) with Cp,m=3.502R, 3.466R, and 4.217R for N2(g), H2(g), and NH2(g), respectively. From this information, calculate delta H of NH3(g) at 375 K. Assume thaat the heat capacities are independent of temperature.

Calculate $\Delta H$ for the reaction: $$ 2 \mathrm{NH}_{3}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{H}_{2} \mathrm{O}(l) $$ given the following data: $$ 2 \mathrm{NH}_{3}(g)+3 \mathrm{N}_{2} \mathrm{O}(g) \longrightarrow 4 \mathrm{N}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l) $$ $\Delta H=-1010 . \mathrm{kJ}$ $$ \mathrm{N}_{2} \mathrm{O}(g)+3 \mathrm{H}_{2}(g) \longrightarrow \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{H}_{2} \mathrm{O}(l) $$ $\Delta H=-317 \mathrm{kJ}$ $$ \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ $\Delta H=-623 \mathrm{kJ}$ $$ \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l) $$ $\Delta H=-286 \mathrm{kJ}$

Question

At 1000.K, delta H=-123.77 Kj/mol for the reaction N2(g) + #H2(g) -> 2NH3(g) with Cp,m=3.502R, 3.466R, and 4.217R for N2(g), H2(g), and NH2(g), respectively. From this information, calculate delta H of NH3(g) at 375 K. Assume thaat the heat capacities are independent of temperature.

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