The enthalpy change for the combustion of `N_(2)H_(4)(l)` (Hydrazine) is `-622.2 kJ mol^(-1)`. The products are `N_(2)(g)` and `H_(2)O(l)`. If `Delta_(f)H^(Theta)` for `H_(2)O(l) is -285.8 kJ mol^(-1)`. The `Delta_(f)H^(Theta)` for hydrazine is

Options

A. `-336.4 kJ mol^(-1)`
B. `+50.6 kJ mol^(-1)`
C. `-622.2kJ mol^(-1)`
D. `+336.4 kJ mol^(-1)`

Explanation

To find the standard enthalpy of formation (Δ_fH°) for hydrazine (N₂H₄), we can use the given enthalpy change for the combustion reaction and the enthalpy of formation for water.

### Step-by-Step Solution:

1. **Write the combustion reaction for hydrazine (N₂H₄)**:
The balanced equation for the combustion of hydrazine in the presence of oxygen is:
\[
N_2H_4(l) + O_2(g) \rightarrow N_2(g) + 2 H_2O(l)
...