For the reaction where Δn=-1Δn=-1, what happens after in increase in volume?? KQ>K so the reaction shifts toward reactants. For the reaction where Δn=0Δn=0, what happens after in increase in volume?? KQ>K so the reaction shifts toward reactants. For the reaction where Δn=+1Δn=+1, what happens after in increase in volume?? KQ>K so the reaction shifts toward reactants.

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Chemistry

Sunshine

25 July, 13:51

For the reaction where Δn=-1Δn=-1, what happens after in increase in volume?? KQ>K so the reaction shifts toward reactants. For the reaction where Δn=0Δn=0, what happens after in increase in volume?? KQ>K so the reaction shifts toward reactants. For the reaction where Δn=+1Δn=+1, what happens after in increase in volume?? KQ>K so the reaction shifts toward reactants.

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Kendra Austin · Answer 1

In general, an increase in pressure (decrease in volume) favors the net reaction that decreases the total number of moles of gases, and a decrease in pressure (increase in volume) favors the net reaction that increases the total number of moles of gases.

Δn = b - a

Δn = moles of gaseous products - moles of gaseous reactants

Therefore, after the increase in volume:

If Δn = - 1 ⇒ there are more moles of gaseous reactants than gaseous products. The equilibrium will be shifted towards the products, that is, from left to right, and K>Q. If Δn = 0 ⇒ there is the same amount of gaseous moles, both in products and reactants. The system is at equilibrium and K=Q. Δn = + 1 ⇒ there are more moles of gaseous products than gaseous reactants. The equilibrium will be shifted towards the reactants, that is, from right to left, and K