In order to find the factors that will shift the reaction towards right, we first analyze the given reaction. According to the given data the reaction is exothermic in nature.
Hence based on this information we have to find which of the given factors will shift the equilibrium towards right.
According to Le-Chatlier's principle if the concentration of the products is decreased the system tries to increase the concentration by favoring the forward reaction. Hence by removing H2 the equilibrium will shift towards right.
Similarly, when the concentration of the reactants is increased the system tries to decrease its concentration by favoring the forward reaction. Hence by adding water the equilibrium will shift towards right.
According to the Le-Chatlier's principle we know that an exothermic reaction is favored if the temperature is decreased. Hence as the temperature is decreased the forward reaction is favored. Hence by cooling the concentration of the products will increase. This implies that cooling will shift the equilibrium towards right.
According to the Le-Chatlier's principle we know that when the concentration of the products is increased the system tries to decrease the concentration of the products by favoring the backward reaction. Hence by adding CO2 the equlibrium will shift towards left.
Similarly, when the volume is decreased the equilibrium will shift towards the side of the reaction with fewer moles. In this case there are equal number of moles on either side hence the equilibrium will not shift on either side.
By adding the catalyst the equilibrium will not shift on either side because the catalyst will not favor only forward reaction but also favor the backward reaction by same rate.
From Le-Chtlier's principle we know that the forward reaction of an exothermic reaction will be favored only when the temperature is decreased. Hence by increasing the temperature the reaction will be favored in the backward direction. Hence by increasing the temperature the equilibrium will shift on the left.
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