Diborane isa potential rocket fuel that undergoes combustion according to the reaction,
`B_(2)H_(6)(g) +3O_(2)(g) rarr B_(2)O_(3)(g) +3H_(2)O(g)`
From the following data, calculate the enthalpy change for the combustion of diborane:

Options

A. `2B(s) +((3)/(2)) O_(2)(g) rarr B_(2)O_(3)(s), DeltaH^(Theta) =- 1273 kJ mol^(-1)`
B. `H_(2)(g) +((1)/(2))O_(2)(g) rarr H_(2)O(l), DeltaH^(Theta) =- 286 kJ mol^(-1)`
C. `H_(2)O(l) rarr H_(2)O(g),DeltaH = 44 kJ mol^(-1)`
D. `2B(s) +3H_(2)(g) rarr B_(2)H_(6) (g) , DeltaH^(Theta) = 36 kJ mol^(-1)`

Explanation

To calculate the enthalpy change for the combustion of diborane (B₂H₆), we will use Hess's law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for the individual steps of the reaction. We will use the given reactions and their enthalpy changes to derive the enthalpy change for the combustion of diborane.

### Step-by-Step Solution:

1. **Write the combustion reaction:**
The combustion of diborane can be represented as:
\[
B_2H_6(g) + 3O_2(g) \rightarrow B_2O_3(g) + 3H_2O(g)
...