the 1.
For reaction A(g) + 2B(g) 2C(g) + 2D(g)
5.
The equilibrium constant, Kp, for the reaction CO(g) + H2O(g) CO2(g) + H2(g)
the following data was collected at constant temperature. Determine the correct rate law for this reaction. Trial 1 2 3 4 A. B. C. D. E. 2. Initial [A] (mol/L) 0.125 0.375 0.250 0.375 Rate = k[A] [B] Rate = k[A]2 [B] Rate = k[A] [B]2 Rate = k[A] Rate = k[A]3 6. The decomposition of SOCl2 is first-order in SOCl2. If the half-life for the reaction is 4.1 hr, how long would it take for the concentration of SOCl2 to drop from 0.36 M to 0.045 M? A. B. C. D. E. 3. 0.52 hr 1.4 hr 12 hr 33 hr > 40 hr Initial [B] (mol/L) 0.200 0.200 0.400 0.400 Initial Rate (mol/(Lmin)) 7.25 21.75 14.50 21.75
at 986 C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium? A. Yes. B. No, the forward reaction must proceed to establish equilibrium. C. No, the reverse reaction must proceed to establish equilibrium. D. The volume of the container must be known before deciding. E. The starting concentrations of all substances must be known before deciding. A mixture 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium of concentration COBr2 was 0.233 M. What is the value of Kc for this reaction? CO(g) + Br2(g) A. B. C. D. E. 7. 5.23 1.22 1.165 0.858 0.191 COBr2(g)
Ammonia will react with oxygen in the presence of a copper catalyst to form nitrogen and water. From 164.5 C to 179.0 C, the rate constant increases by a factor of 4.27. What is the activation energy of this oxidation reaction? A. B. C. D. E. 24.5 kJ/mol 165 kJ/mol 242 kJ/mol 1630 kJ/mol > 104 kJ/mol
The equilibrium constant Kc for the reaction A(g) + B(g) C(g)
is 0.76 at 150 C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150 C, what will be the equilibrium concentration of C? A. B. C. D. E. 8. 0.19 M 0.29 M 0.36 M 0.41 M 0.51 M
4.
Hydrogen sulfide will react with water as shown in the following reactions.
H2S(g) + H2O(l) H3O+(aq) + HS-(aq) K1 = 1.0 x 10-7 HS-(aq) + H2O(l) H3O+(aq) + S2-(aq) K2 = ?? H2S(g) + 2H2O(l) 2H3O+(aq) + S2-(aq) K3 = 1.3 x 10-20 What is the value of K2? A. B. C. D. E. 1.3 2.3 1.3 7.7 7.7 10-27 10-7 10-13 1012 1026
If 2.00 mol of H2 and 1.00 mol of I2 come to equilibrium at this temperature (458C), how many moles of HI will be in the final mixture? (First, consider this question: Why is the volume of the container not needed for this problem?) H2(g) + I2(g) 2HI(g) Kc = 50.3 at 458C
Answers: 1. D 2. C 3. B 4. C
5. 6. 7. 8.
B A A 1.87 mol HI