Question

Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after a decrease in pressure or volume. If there is no change in the concentration of the species, leave the box blank. CH 4 ( g ) + 2 H 2 S ( g ) − ⇀ ↽ − CS 2 ( g ) + 4 H 2 ( g ) after decreasing the pressure after decreasing the volume of the reaction vessel

Answer 1

CH​​​4  ( g ) + 2 H 2S ( g ) ----------> CS​​​​​2 ( g ) + 4 H​​​​​2 (g)

This can be explained by  Le chatelier's principal.

it stats that if there is a change in temperature, pressure, moles, volume etc in a chemical reaction at equilibrium, then reaction tries to restablise equilibrium by shifting to oppose the change.

Effect of pressure..

if we decrease the pressure,the equilibrium will shift towards that side of reaction which have more moles of gas. So in case of above reaction concentration of CS2 and H2 will increase because it have more moles of gases

In case of pressure increase ,the concentration of product will increase .

Effect of volume ..

If we decrease the volume the equilibrium will shift to that side which have less number of moles of gases .

In above reaction concentration of CH 4 and H2S will increase as product side have less mole .

In case of increase in volume, the equilibrium will shift towards more number of moles.

Note:-

All these happens at constant temperature

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