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# the sulfur dioxide or oxygen

The ratio in the balanced equation is 1:3:21:3:2. That is, for every 11 moleculemolecule of N2 gasN2 gas there are 33 moleculesmolecules of H2 gasH2 gas and 22 moleculesmolecules of NH3 gasNH3 gas (from the balanced equation). Therefore the ratio is 4 molecules of reactant gas4 molecules of reactant gas to 2 molecules of product gas2 molecules of product gas.

• An increase in pressure will:
• Favour the reaction that decreases the number of gas molecules.
• There are fewer molecules of product gasfewer molecules of product gas than reactant gas, so the forward reaction is favoured.
• The equilibrium will shift to the right and the yield of NH3NH3 will increase.
• decrease in pressure will:
• Favour the reaction that increases the number of gas molecules.
• There are more molecules of reactant gasmore molecules of reactant gas, so the reverse reaction is favoured.
• The equilibrium will shift to the left and the yield of NH3NH3 will decrease.

Consider illustration in Figure 8.2.

Figure 8.2 shows how changing the pressure of a system results in a shift in the equilibrium to counter that change. In the original system there are 12molecules in total: 6H2+2N2⇋4NH36H2+2N2⇋4NH3

If you decrease the pressure (shown by an increase in volume), the equilibrium will shift to increase the number of gas molecules. That shift is to the left and the number of H2H2 and N2N2 molecules will increase while the number of NH3NH3 molecules will decrease:

If you increase the pressure (shown by a decrease in volume), the equilibrium will shift to decrease the number of gas molecules. That shift is to the right and the number of H2H2 and N2N2 molecules will decrease while the number of NH3NH3 molecules will increase:

Note that the total number of nitrogen and hydrogen atoms remains the same in all three situations. Equations (a) and (b) are not balanced equations.

Another example is the reaction between sulfur dioxide and oxygen: