For the reversible reaction, The equilibrium shifts in the forward direction [2014]

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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 the forward direction [2014]

1 by increasing the concentration of $N H_{3 (g)}$

2 by decreasing the pressure

3 by decreasing the concentrations of $N_{2 (g)}$ and $H_{2 (g)}$

4 by increasing pressure and decreasing temperature

Ans.
(4)

As the forward reaction is exothermic and leads to lowering of pressure (produces lesser number of gaseous moles) hence, according to Le Chatelier’s principle, at high pressure and low temperature, the given reversible reaction will shift in forward direction to form more product.

Solution

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 the forward direction [2014]

1 by increasing the concentration of $N H_{3 (g)}$

2 by decreasing the pressure

3 by decreasing the concentrations of $N_{2 (g)}$ and $H_{2 (g)}$

4 by increasing pressure and decreasing temperature

Ans.
(4)

As the forward reaction is exothermic and leads to lowering of pressure (produces lesser number of gaseous moles) hence, according to Le Chatelier’s principle, at high pressure and low temperature, the given reversible reaction will shift in forward direction to form more product.

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Solution

Q. For the reversible reaction, N2(g)+3H2(g)⇌2NH3(g)+heat The equilibrium shifts in the forward direction [2014]

1 by increasing the concentration of NH3(g)

2 by decreasing the pressure

3 by decreasing the concentrations of N2(g) and H2(g)

4 by increasing pressure and decreasing temperature

Ans. (4) As the forward reaction is exothermic and leads to lowering of pressure (produces lesser number of gaseous moles) hence, according to Le Chatelier’s principle, at high pressure and low temperature, the given reversible reaction will shift in forward direction to form more product.

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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 the forward direction [2014]

1 by increasing the concentration of $N H_{3 (g)}$

3 by decreasing the concentrations of $N_{2 (g)}$ and $H_{2 (g)}$

Ans.
(4)

As the forward reaction is exothermic and leads to lowering of pressure (produces lesser number of gaseous moles) hence, according to Le Chatelier’s principle, at high pressure and low temperature, the given reversible reaction will shift in forward direction to form more product.