Each of the following reactions is allowed to come to equilibrium and then the volume is changed as indicated. predict the effect (shift right, shift left, or no effect) of the indicated volume change. drag the appropriate items to their respective bins. co(g) + h2o(g) < => co2(g) + h2(g) (volume is decreased) pcl3(g) + cl2(g) < => pcl5(g) (volume is increased) caco3(s)< => cao(s) + co2(g) (volume is increased)

No net shift in the reactants and products is an equilibrium constant. In the first reaction, there is no effect, in second shifts to the left and third shifts to right.

Equilibrium shift can be explained by the rules of Le and the change in the volume affects the system as the number of the particles gets varied.

For the first reaction when the volume is decreased then the pressure will increase then the equilibrium will shift towards the fewer and then more number of the gas moles and hence, will have no net effect.

In the second reaction when the volume is increased then the pressure will decrease and the reaction will shift towards more moles of the gas present that is the left side.

In the third reaction, when the volume is increased then the pressure will decrease and the equilibrium will shift towards the side where more moles are present. Hence the increase in the volume will shift the equilibrium towards the right.

Therefore, a decrease in volume will have no effect, while the increase in volume will shift the reaction towards the left and right.

Learn more about the equilibrium constant here:

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