$N_{2 (g)} + 3 H_{2 (g)} \leftrightarrow 2 N H_{3 (g)}$ If some $H C l$ gas is passed into the reaction mixture at the equilibrium of this reaction,then :

Equilibrium position shifts towards left

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Equilibrium position shifts towards right

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Concentration of

H_{2}

increases

No worries! We‘ve got your back. Try BYJU‘S free classes today!

The equilibrium position is not affected

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A Equilibrium position shifts towards left
$N_{2 (g)} + 3 H_{2 (g)} \leftrightarrow 2 N H_{3 (g)}$

Hydrogen ions are on the right hand side of the equilibrium therefore the equilibrium will shift to the left hand side to compensate resulting in higher concentration of reactants.
Option A is correct because both hydrogen and chloride ions are added.

Suggest Corrections

Similar questions

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g) + h e a t

Given the reaction shown above, which change will not shift the equilibrium position for the reaction?

Q. For the reversible reaction :

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g) + h e a t

The equilibrium shifts in forward direction-

N_{2} (g) + {3 H}_{2} (g) ⇌ 2 {N H}_{3} (g) + h e a t

The reaction above is carried out in a sealed vessel.
Which changes would both shift the equilibrium position to favor in the formation of products?

Q. Assertion (A): Increase of pressure for a reaction which is in equilibrium shifts the equilibrium towards direction where less number of moles are present.
Reason (R): The change in pressure in an equilibrium reaction changes the position or direction of equilibrium.

A mixture of 1.57 mol of $N_{2}$ , 1.92 mol of $H_{2}$ and 8.13 mol of $N H_{3}$ is introduced into a 20 L reaction vessel at 500 K. At this temperature, the equilibrium constant, $K_{c}$ for the reaction
$N_{2} (g) + 3 H_{2} (g) \leftrightarrow 2 N H_{3} (g) i s 1.7 \times 10^{2}$
Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

Join BYJU'S Learning Program

N2(g)+3H2(g)↔2NH3(g) If some HCl gas is passed into the reaction mixture at the equilibrium of this reaction,then :

$N_{2 (g)} + 3 H_{2 (g)} \leftrightarrow 2 N H_{3 (g)}$ If some $H C l$ gas is passed into the reaction mixture at the equilibrium of this reaction,then :