For the reaction N 2 g -3 H 2 g - 2 NH 3 g - - H -93-6 kJ mol -1 - The concentration of H 2 at equilibrium will increase ifA- the temperature is decreasedB- the volume of the system is decreasedC- N 2 is added at constant volumeD- NH 3 is added

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Equilibrium Constant and Standard Free Energy Change

For the react...

Question

For the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g), △ H = - 93.6 k J m o l^{- 1} .$ The concentration of $H_{2}$ at equilibrium will increase if

the temperature is decreased

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the volume of the system is decreased

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N_{2}

is added at constant volume

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N H_{3}

is added

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Solution

The correct option is D $N H_{3}$ is added
From Le-chatelier principle,
For an exothermic reaction, the heat of reaction will be released, if temperature is increased the reaction will shift in backward direction and favour reactant.
When the volume of the system is increase, the reaction will shift to that direction which have lower number of moles.
Simlarly, if reactants ( $N_{2} a n d H_{2}$ is added the reaction will shift towards forward reaction.
and if $N H_{3}$ (g) is added the reaction will shift toward the production of reactants

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Similar questions

For the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g), Δ H = - 93.6 k J m o l^{- 1}$ . The amount (i.e. number of mole) of~ $H_{2}$ at equilibrium will
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For the reaction $2 N H_{3} (g) ⇌ N_{2} (g) + 3 H_{2} (g), Δ H = 93.6 k J m o l^{- 1}$ . Which of the following is incorrect?

For the reaction $2 N H_{3} (g) ⇌ N_{2} (g) + 3 H_{2} (g), Δ H = 93.6 k J m o l^{- 1}$ . Which of the following facts does not hold well?

Q. A gaseous catalyst X is added in a equilibrium mixture of

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For the reaction N2(g)+3H2(g)⇌2NH3(g),△H=−93.6 kJ mol−1. The concentration of H2 at equilibrium will increase if

For the reaction $N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g), △ H = - 93.6 k J m o l^{- 1} .$ The concentration of $H_{2}$ at equilibrium will increase if