Answer:
An increase in pressure favors the side with fewer particles but has no effect if both sides have the same number of particles.
Explanation:
Answer:
1. Favours the forward reaction
2. Favours the backward reaction
3. No effect
4. No effect
5. No effect
Explanation:
An increase in pressure will cause the reaction to proceed towards the side having a low volume according to Le Chatelier's principle. But, pressure will only have effects if one of the reactant and one of the product is a gas, and will not have effect if the total volume of the reactants and products are the same. So let us attempt the questions above with these understanding:
1. N2(g) + 3H2(g) → 2NH3(g)
Total Volume of reactants = 1 + 3 = 4
Total volume of product = 2
An increase in pressure will favours the forward reaction since it has a lower volume.
2. 2SO3(g) → 2SO2(g) + O2(g)
Total Volume of reactant = 2
Total volume of products = 2 + 1 = 3
An increase in pressure will favours the Backward reaction since it has a lower volume.
3. SnO2(s) + 2H2(g) → Sn(s) + 2H20(g)
Total Volume of gaseous reactant = 2
Total volume of gaseous product = 2
An increase in pressure will have no effect, since the volume of the gaseous reactant and product are the same
4. Na2CO3(s) + 2HCl(aq) → CO2(g) + H2O(l) +2NaCl(aq)
An increase in pressure will have no effect since there is no gaseous reactant
5. AgNO3(aq) + Cu(s) → CUNO3(aq) + Ag(s)
An increase in pressure will have no effect since there are no gaseous reactants nor products
