Question

applying Leonard Chateliers principal which direction will the equilibrium shift in the following reaction CH4 (g)...

applying Leonard Chateliers principal which direction will the equilibrium shift in the following reaction
CH4 (g) + 2O2 (g) = CO2 (g) + 802.3 kj

(a) if the temperature is increased
(b) if a catalyst is added
(c) if CH4 is added
(d) if the volume of the reaction vessel is decreased

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Homework Answers

Answer #1

a) Increase in temperature in endothermic reactions favours backward or reverse direction that is towards reactants.

b) if catalyst is added there will be no change in equilibrium as the catalyst has no effect on reaction.

c) If CH4 is added, the equilibrium will move in forward direction in order to decrease the increased amount of CH4.

d) If the volume is decreased the pressure of the reaction vessel increases. As pressure is increased the equilibrium will move in that direction in which the number of moles of gaseous reactants are less.

In this reaction, the number of gaseous molecules on left side are 3 and on right side are 1 so the equilibrium will move in forward direction that is towards products.

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