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.

Explanation:

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<Q.

No table found. the question asks for covalent bond based on electronegativies