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4. How the reaction conditions (T and P) should be changed in order to shift the...

4. How the reaction conditions (T and P) should be changed in order to shift the equilibrium
CO (gas) + H2O (gas) CO2 (gas) + H2 (gas) if ΔН0800K = -36.994 KJ/mol.
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Answer #1

Reaction:

CO(g) +H2O(g) <----> CO2(g) +H2(g)

Since number of moles of gas are equal in both reactant and product side

Therefore, no effect of changing the pressure on equilibrium.i.e. equilibrium will not shift on changing the pressure.

Also ∆H° for the reaction is negative(-36.994 KJ/mol) implies the reaction is exothermic reaction.

Therefore for exothermic reactions by Le Chatelier's principle:

Increase in temperature will result the reaction to shift in backward direction. That is on increasing temperature more CO and H2O will be produced.

Decrease in temperature will result the reaction to shift in forward direction. That is on decreasing temperature more CO2 and H2 will be produced.

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