Question

Diborane is a potential rocket fuel which undergoes combustion according to the reaction. $B_2H_6 (g) + 3 O_2 (g) \rightarrow B_2O_3 (s) + 3H_2O (g)$
From the following data, calculate the enthalpy change for the combustion of diborane.
$2B(s) + \frac{3}{2} O_2 (g) \longrightarrow B_2O_3(s)$ $\Delta H$ = –1273 kJ mol⁻¹
$H_2(g)+ \frac{1}{2} O_2(g) \longrightarrow H_2O(l)$ $\Delta H$ = – 286 kJ mol⁻¹
$H_2O(l) \longrightarrow H_2O(g)$ $\Delta H$ = 44 kJ mol⁻¹
$2B(s)+ 3H_2 (g ) \longrightarrow B_2H_6 (g)$ $\Delta H$ = 36 kJ mol⁻¹

Answer 1

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