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10. Show how the forward and reverse reaction rates respond to a sudden increase in the temperature of the system below at t1. Use a solid line for the forward rate and a dotted line for the reverse rate. The system restores equilibrium at t2. The arrow diagram on the right is another way of depicting the same information. You may use it to do your rough work. ΔH = –603 kJ/mol Ni(s) + 4 CO(g) Ni(CO)4(g)
Rate
Ei
S
Ef t1
Time
t2
11. Co(H2O)62+(aq) + 2 Cl−(aq) pink
Co(H2O)4Cl2(aq) + 2 H2O(l) purple
A flask containing the above equilibrium turns from purple to pink when cooled. State whether the forward reaction is endothermic or exothermic. Explain how you arrived at your answer.
Concentration
12. A + B
AB + 16.8 kJ/mol
AB
B A t1
t2 Time
(a) In which direction is the equilibrium system shifting?
(b) What specifically was done to this system at t1?
100 Chapter 2 Chemical Equilibrium
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