In a container of constant volume at a particular temparature `N_(2)` and `H_(2)` are mixed in the molar ratio of `9:13`. The following two equilibria are found o be coexisting in the container
`N_(2)(g)+3H_(2)(g)harr2NH_(3)(g)`
`N_(2)(g)+2H_(2)(g)harr N_(2)H_(4)(g)`
The total equiibrium pressure is found to be `305` atm while partial pressure of `NH_(3)(g)` and `H_(2)(g)` are `0.5` atm and `1` atm respectivly. Calculate of equilibrium constants of the two reactions given above.

Explanation

To solve the problem step by step, we will calculate the equilibrium constants for the two reactions given the information provided.

### Step 1: Define the Initial Conditions
Given that nitrogen (N₂) and hydrogen (H₂) are mixed in a molar ratio of 9:13, we can express their partial pressures in terms of a variable \( p \):
- Let the partial pressure of nitrogen \( P_{N_2} = 9p \)
- Let the partial pressure of hydrogen \( P_{H_2} = 13p \)

### Step 2: Write the Total Pressure Equation
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