# For the reversible reaction :N2(g) + 3H2(g) 2NH3(g) + heatThe equilibrium shifts in forward direction : Option 1) by increasing the concentration of NH3(g) Option 2) by decreasing the pressure Option 3) by decreasing the concentration of N2(g) and H2(g) Option 4) by increasing pressure and decreasing temperature

As we learnt in

Effect of Pressure change -

A pressure change obtained by changing the volume can affect the yield of product in case of a gaseous reaction where the total number of moles of gaseous reactant and total number of moles of gaseous product are different.

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Equilibrium constant and sign of Enthalpy Change -

The equilibrium constant for an exothermic reaction ( negative $\bigtriangleup H$ ) decreases as the temperature increases.

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In the given reaction , Stoichiometric moles of product < Stoichiometric moles of reactants.

According to Le Chatelier's  principles upon increasing pressure, the reaction will proceed in forward direction.

Also upon decreasing temperature, for an exothermic reaction, the reaction should push forward.

Option 1)

by increasing the concentration of NH3(g)

Incorrect

Option 2)

by decreasing the pressure

Incorrect

Option 3)

by decreasing the concentration of N2(g) and H2(g)

Incorrect

Option 4)

by increasing pressure and decreasing temperature

Correct

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