The net rate of reaction of the change :
`[Cu(NH_(3))_(4)]^(2+)+H_(2)O ?" "[Cu(NH_(3))_(3)H_(2)P]^(2+)+NH_(3)` is,
`(dx)/(dt) =2.0xx10^(-4)[Cu(NH_(3))_(4)]^(2+)-3.0xx10^(5)[Cu(NH_(3))_(3)H_(2)O]^(2+)[NH_(3)]`
Calculate :
rate expression for forward and backward reactions.

Explanation

To solve the problem, we need to derive the rate expressions for both the forward and backward reactions based on the given net rate of reaction. Let's break down the steps:

### Step 1: Understand the Net Rate of Reaction
The net rate of reaction is given by the equation:
\[ \frac{dx}{dt} = k_F [\text{Reactants}] - k_B [\text{Products}] \]
where \( k_F \) is the rate constant for the forward reaction and \( k_B \) is the rate constant for the backward reaction.
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