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Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium, 22% of the NOBr decomposes. What is the equilibrium constant, Kp, for the reaction?

Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium, 22% of the NOBr decomposes. What is the equilibrium constant, Kp, for the reaction?

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Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium, 22% of the NOBr decomposes. What is the equilibrium constant, Kp, for the reaction?
initially present in a 1.OL flask at 25 °C, what change in concentrations (if any) will occur in time? 5. Consider the reaction A(aq) t 2 B(aq) where K,-4.1 at 25 "C, If 0.50 M A(aq) and 1.5 M B(sq) are CHEM 102 Equilibrium Study Guide [A] will decrease and [B] will decrease. 76. [A] will decrease and [B] will increase. a. [A] will increase and [B] will decrease. d. [A] will increase and [B] will increase. c. 29 [A] and [B] remain unchanged. e. 0. An aqueous mixture of hydrocyanie acid and ammonia bas initial concentrations of 0.100 M HICNGRD 0.140 M NH3(aq). At equilibrium, the CN (ag) concentration is 0.055 M. Calculate K for the reaction. HCN(aq) + NH3(aq) = CN (aq) + NH,'(aq) 0.22 b. a. 0.79 c. 1.5 d. 3.9 e. 14 7. Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 0.260 atm of NOB is sealed in a flask and allowed to reach equilibrium, 22% of the NOBI decomposes. What is the equilibrium constant, Kp, for the reaction? 2.3 x 10-3 b. 4.5 x 10 з 3.5 x 10-2 d. 4.8 x 10-2 8.0 x 10-2 a. с. e. 8. The equilibrium constant, Kc, for the following reaction is 1.0 x 10 at 1500 K. If 0.570 M N2 and 0.570 M O2 are allowed to equilibrate at 1500 K, what is the concentration of NO? 5.7 x 106 M N2(g) + O2(g) =2 NO(g) а. b. 9.0 x 104M 2.4 x 104 M 1.8 x 10-3 M 2.4 x 10-3 M с. d. e. The equilibrium constant (K.) for the following reaction is 6.7 x 10-10 at 630 °C. N2(s) + O2(g) =2 NO(g) What is the equilibrium constant for the reaction below at the same temperature? NO(g) = 1/2 N2(g) + 1/2 O2(g) a. 3.9 x 104 b. 5.5 x 104 c. 7.5 x 108 d. 1.5 x 10° 3.0 x 10° e.
Transcribed Image Text:initially present in a 1.OL flask at 25 °C, what change in concentrations (if any) will occur in time? 5. Consider the reaction A(aq) t 2 B(aq) where K,-4.1 at 25 "C, If 0.50 M A(aq) and 1.5 M B(sq) are CHEM 102 Equilibrium Study Guide [A] will decrease and [B] will decrease. 76. [A] will decrease and [B] will increase. a. [A] will increase and [B] will decrease. d. [A] will increase and [B] will increase. c. 29 [A] and [B] remain unchanged. e. 0. An aqueous mixture of hydrocyanie acid and ammonia bas initial concentrations of 0.100 M HICNGRD 0.140 M NH3(aq). At equilibrium, the CN (ag) concentration is 0.055 M. Calculate K for the reaction. HCN(aq) + NH3(aq) = CN (aq) + NH,'(aq) 0.22 b. a. 0.79 c. 1.5 d. 3.9 e. 14 7. Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 0.260 atm of NOB is sealed in a flask and allowed to reach equilibrium, 22% of the NOBI decomposes. What is the equilibrium constant, Kp, for the reaction? 2.3 x 10-3 b. 4.5 x 10 з 3.5 x 10-2 d. 4.8 x 10-2 8.0 x 10-2 a. с. e. 8. The equilibrium constant, Kc, for the following reaction is 1.0 x 10 at 1500 K. If 0.570 M N2 and 0.570 M O2 are allowed to equilibrate at 1500 K, what is the concentration of NO? 5.7 x 106 M N2(g) + O2(g) =2 NO(g) а. b. 9.0 x 104M 2.4 x 104 M 1.8 x 10-3 M 2.4 x 10-3 M с. d. e. The equilibrium constant (K.) for the following reaction is 6.7 x 10-10 at 630 °C. N2(s) + O2(g) =2 NO(g) What is the equilibrium constant for the reaction below at the same temperature? NO(g) = 1/2 N2(g) + 1/2 O2(g) a. 3.9 x 104 b. 5.5 x 104 c. 7.5 x 108 d. 1.5 x 10° 3.0 x 10° e.
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