The following reaction attains equillibrium at high temperatures-N 2 g -2 H 2 O g - heat - 2 NO g -2 H 2 g The concentration of NO g is affected by-A- Increasing the nitrogen concentrationB- Decreasing the hydrogen concentrationC- Compressing the reaction mixtureD- Addition of a catalyst

The correct options are A Increasing the nitrogen concentration nbsp; B Decreasing the hydrogen concentration C Compressing the reaction mixture nbsp;Accord ...

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Byju's Answer

Standard XII

Chemistry

Characteristics of Equilibrium Constant

The following...

Question

The following reaction attains equillibrium at high temperatures:
$N_{2} (g) + 2 H_{2} O (g) + h e a t ⇌ 2 N O (g) + 2 H_{2} (g)$
The concentration of $N O (g)$ is affected by:

Increasing the nitrogen concentration

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Decreasing the hydrogen concentration

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Compressing the reaction mixture

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Addition of a catalyst

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Solution

The correct options are
A Increasing the nitrogen concentration
B Decreasing the hydrogen concentration
C Compressing the reaction mixture
According to Le-Chatelier's principal in the above reaction,
Increasing the nitrogen concentration and decreasing the hydrogen concentration will result in a forward reaction. Compressing the reaction mixture means that we are decreasing the volume, which will result in an increase in the concentration and hence the reaction will shift in the direction where gaseous moles is less. So, the reaction will move backwards.
Addition of catalyst will help to achieve equillibrium faster. It doesnt affect the concentration of the reactant or the product.

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The following reaction attains equillibrium at high temperatures: N2(g)+2H2O(g)+heat⇌2NO(g)+2H2(g) The concentration of NO(g) is affected by:

The following reaction attains equillibrium at high temperatures:
$N_{2} (g) + 2 H_{2} O (g) + h e a t ⇌ 2 N O (g) + 2 H_{2} (g)$
The concentration of $N O (g)$ is affected by: