Nitric oxide reacts with bromine and gives nitrosyl-bromide as per reaction given below:
`2NO_((g))+Br_(2(g))hArr2NOBr_((g))`.
When `0.087 "mole"` of `NO` and `0.0437 "mole"` of `Br_(2)` are mixed in a closed container at constant temperature, `0.0518 "mole"` of `NOBr` is obtained at equilibrium. Calculate equilibrium amount of nitric oxide and bromine.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the balanced chemical equation.
The balanced equation for the reaction is:
\[ 2 \text{NO} (g) + \text{Br}_2 (g) \rightleftharpoons 2 \text{NOBr} (g) \]

### Step 2: Set up an ICE table (Initial, Change, Equilibrium).
We will denote the initial moles of NO and Br₂, the change in moles as \( x \), and the equilibrium moles.
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