According to Le Chatelier’s principle, which direction will the equilibrium shift when the following stresses in the following 6 questions are applied to the reaction below, currently at equilibrium? Place a right arrow, left arrow, or zero for no change.
2Ce(IO3)4(aq) + 24H2C2O4(aq)→Ce2(C2O4)3(aq) + 4I2(aq) + 42CO2(g) + 24H2O(l)
1.
Argon gas is added.
2.
Increase the concentration of carbon dioxide.
3.
Decrease the volume.
4.
Increase the concentration of the Ce(IO3)4.
5.
Decrease the concentration of the I2.
6.
Decrease the temperature (the reaction is exothermic).
Write an equilibrium constant expression for each of the following chemical equations. Remember that only (aq) and (g) are kept in the equilibrium constant expression. Do your work on paper and then compare it with my answers.
7.
P4O10(g) + 6PCl5(g) ⇌ 10POCl3(g)
8.
IF(s) ⇌ ½F2(g) + ½I2(g)
9.
2NO3– (aq) + 8H+(aq) + 3Cu(s) ⇌ 2NO(g) + 3Cu2+(aq) + 4H2O(l)
10.
NH2COONH4(g) ⇌ CO2(g) + 2NH3(g)
11.
2PbS(s) + 3O2(g) ⇌ 2PbO(s) + 2SO2(g)
12.
Ni(s) + 4CO(g) ⇌ Ni(CO)4(g)
13.
4HCl(g) + O2(g) ⇌ 2Cl2(g) + 2H2O(g)
14.
NH4HS(g) ⇌ NH3(g) + H2S(g)
1. Zero (Argon is an inert gas and does not affect the equilibrium)
2. Left (Increasing the concentration of product CO2 will shift the equilibrium towards the reactants to counteract the increase)
3. Left (Decreasing the volume will cause the equilibrium to shift towards the side with fewer moles of gas in order to decrease the pressure)
4. Right (Increasing the concentration of reactant Ce(IO3)4 will shift the equilibrium towards the products)
5. Right (Decreasing the concentration of product I2 will shift the equilibrium towards the products to counteract the decrease)
6. Right (Decreasing the temperature of an exothermic reaction will shift the equilibrium towards the products to increase the heat)
7. Kc = [POCl3]^10 / [P4O10][PCl5]^6
8. Kc = [F2]^(1/2)[I2]^(1/2) / [IF]
9. Kc = [NO]^2[H2O]^4[Cu2+]^3 / [NO3-]^2[H+]^8[Cu]^3
10. Kc = [NH3]^2[CO2] / [NH2COONH4]
11. Kc = [PbO]^2[SO2] / [PbS]^2[O2]^3
12. Kc = [Ni(CO)4] / [Ni][CO]^4
13. Kc = [Cl2]^2[H2O]^2 / [HCl]^4[O2]
14. Kc = [NH3][H2S] / [NH4HS]