1. Tardigrade
  2. Question
  3. Chemistry
  4. Nitric oxide reacts with Br2 and gives nitrosyl bromide as reaction given below: 2 NO (g)+ Br 2(g) leftharpoons 2 NOBr (g) When 0.087 mol of NO and 0.0437 mol of Br 2 are mixed in a closed container at constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. The equilibrium amount of NO is

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Q. Nitric oxide reacts with $Br_2 $ and gives nitrosyl bromide as reaction given below :
$2 NO _{(g)}+ Br _{2(g)} \rightleftharpoons 2 NOBr _{(g)}$
When $0.087$ mol of $NO$ and $0.0437 mol$ of $Br _{2}$ are mixed in a closed container at constant temperature, $0.0518 mol$ of $NOBr$ is obtained at equilibrium. The equilibrium amount of $NO$ is

Equilibrium

Solution:

$2 NO _{(g)}+ Br _{2(g)} \rightleftharpoons 2 NOBr _{(g)}$
$\begin{array}{lccl}\text { Initial moles } & 0.087 & 0.0437 & 0 \\ \text { Moles at eq. } & (0.087-2 x) & (0.0437-x) & 2 x\end{array}$
But $2x = 0.0518 .-. x = 0.0259 $
$(n_No)_eq = 0.087 - 0.0518 = 0.0352\, mol $