4 (6 pts) For the reaction 2 H (g)+ O (0)2HO (g)highly exothermic what will happ

Question

4 (6 pts) For the reaction 2 H (g)+ O (0)2HO (g)highly exothermic what will happen to the equilibrium (to the relative amounts of reactants products) if a 1,12] is and b. the temperature is increased c. the pressure is decreased she LefT 544 pts) For each [Hon below, give them! TaKe Loom 56 a. 6.4 10-8 M 0 4 By oor oeh 101] below, give the thg a. 9.5x 106 b. 7.5 x1 7. (4 ptsf Foreach pH below, givethe [H30 7raise lo'rn-# a. 7.4 b. 3.8 TaKegwa2 8. (4 pts) Give the conjugate base for each acidbelow. a. H2P b. HNO3 H P 1 H 9. (4 pts) Give the conjugate acid for each base below. a. H2N- Add b. PH H3 N 10.(4 pts) Identify which reactant is the acid and which is the base in each reaction below. a. NH3 + HF NH4+ + F. Aia Base

Explanation / Answer

4. a) According to Le Chatelier principle, on increasing the concentration of reactant, the reaction moves in forward direction in order to undo the effect. So, when [H2] is increased, the reaction will move in forward direction.

b) The forward reaction is exothermic. So, on increasing the temperature, the reaction will move in reverse direction as the reverse reaction is endothermic and it will try to decrease the increase in temperature.

c) On the reactant side, there are 3 moles of gases in total and on the product side, there are 2 moles of gases in total. So, on decreasing the pressure, the reaction will move in the direction on which there are more number of moles of gases, so that the pressure of the system could increase. So, the reaction will move in reverse direction.

5. a) [H3O+] = 6.4*10-8 M

pH = -log[H3O+] = -log (6.4*10-8) = 7.19

b) [H3O+] = 4.4*10-9 M

pH = -log[H3O+] = -log (4.4*10-9) = 8.36

6. a) [OH-] = 9.5*10-6 M

[H3O+][OH-] = 10-14

[H3O+] = 10-14/(9.5*10-6) = 1.05*10-9 M

b) [OH-] = 7.5*10-4 M

[H3O+][OH-] = 10-14

[H3O+] = 10-14/(7.5*10-4) = 1.33*10-11 M

7. a) pH = 7.4

[H3O+] = 10-7.4 = 3.98*10-8 M

b) pH = 3.8

[H3O+] = 10-3.8 = 1.58*10-4 M

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