Lechatlier principle will be used to explain the concept. As per the principle,

Question

Lechatlier principle will be used to explain the concept. As per the principle, when ever any equilibrium reaction is subjected to any constraint ( i.e change in temperature or pressure ), the reaction proceeds as as to decrease the effect of constraint.

1. The reaction is N2(g)+ 3H2(g) --------->2NH3(g), mole of gaseous reactants = 1(N2)+3(H2)= 4 , moles of gasesous H2= 2

so there are more gaseous moles on the reactant (4) and less gas moles on the products (2). From gas law at constant temperature, PV= nRT becomes P is proportional to no of moles . So an increases in pressure increases no of moles and as per Lechatlier principle, the reaction proceeds in a direction so as to decrease the no of moles. So increased pressure favors formation of ammonia. So the reaction proceeds to the right (A is the correct answer).

2. SO2(g)+ 0.5O2(g)<---> SO3(g), moles of gas reactants = 1+0.5= 1.5, moles of gas products= 1, so there are less no of moles on products and more moles on reactants. So when pressure is increased, as per Lechatlier principle, the reaction proceeds where there is a decrease in moles. So more SO3 is formed. so the reaction proceeds to the right( A is the correct answer).

3. C(s)+ H2O(g)------->CO(g)+ H2(g), moles of gas reactants =1, moles of gas products =2, so there are less no of moles on reactant side. When pressure is increased, the reaction proceeds so as to form more C (s) and H2O(g). The reaction proceeds to the left( B is the correct answer).

Explanation / Answer

Increasing the pressure on the following equilibrium, which way does the equilibrium shift. N2g) 3 H2(g) 15 2 NH B Left D None of the above right Increasing the pressure on the following equilibrium, which way does the SO2(g) C no shift 6 equilibrium shift. ½ O2(g) SOse + B LeftCno shift D None of the above right CH20 ( A right 17Increasing the pressure on the following equilibrium, which way does the equilibrium shift. CO + H2) c mo shint D B Left D None of the above

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