Question

Indicate whether the actions below will shift the following reaction: RIGHT, LEFT or NO CHANGE. Heat + NH4CO2NHz(s) <=> 2 NH3(g) + CO2(g) Increasing the quantity of NH4CO2NH2(s) Removing CO2(g) Increasing the volume of the container Increasing the temperature Adding a catalyst right left no change

Answer 1

According to Le-Chateliers principle when we do any change then reaction will go in that direction to restablish equilibrium.

We are increasing NH4CO2NH2 which is reactant so equilibrium go in right direction to form more product to re-establish equilibrium.

We are decreasing CO2 which is product so reaction will come in right direction to increase amount of product.

In case of increase pressure or decrease volume reaction will move in the direction of lower number of moles...hence reaction will come in the left direction.

Since heat is absorbed during the reaction so it is the endothermic reaction and and endothermic reaction are favoured at higher tempreature...hence on increasing tempreature reaction will go in right direction.

Since catalyst increases the rate of reaction of forward as well backward reaction at a same rate and hence there will be no effect of addition of catalyst