Consider the following reaction: 2NO(g)+Br2(g)⇌2NOBr(g) ,Kp=28.4, at 298 K In a reaction mixture at equilibrium, the...
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Consider the following reaction: 2NO(g)+Br2(g)⇌2NOBr(g) ,Kp=28.4, at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 102 torr and that of Br2 is 134 torr . |
Part A What is the partial pressure of NOBr in this mixture? Express your answer in torrs to three significant figures. |
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Consider the following reaction:
2NO(g)+Br2(g)⇌2NOBr(g) ,Kp=28.4, at 298 K
In a reaction mixture at equilibrium, the...
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K In a reaction mixture at equilibrium, the partial...
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 130 torr and that of Br2 is 146 torr What is the partial pressure of NOBr in this mixture? Express your answer using three significant figures.
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K In a reaction mixture at equilibrium, the partial...
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 101 torr and that of Br2 is 150 torr . What is the partial pressure of NOBr in this mixture? Express your answer using three significant figures.
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K. In a reaction mixture at equilibrium, the partial...
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K. In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br2 is 158 torr . What is the partial pressure of NOBr in this mixture?
Consider the reaction: 2 NO(g) + Br2(g) ↔ 2 NOBr(g) Kp = 28.4 atm-1 at 298 K...
Consider the reaction: 2 NO(g) + Br2(g) ↔ 2 NOBr(g) Kp = 28.4 atm-1 at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 173 Torr and that of Br2 is 142 Torr. What is the partial pressure (in Torr) of NOBr in this mixture? PNOBr = ___ Torr
The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g)...
The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 19.9 L container at 298K contains NOBr at a pressure of 0.297 atm and NO at a pressure of 0.251 atm, the equilibrium partial pressure of Br2 is ? atm.
Consider the following reaction where K. = 154 at 298 K: 2NO(g) + Br2(g) = 2NOBr(g)...
Consider the following reaction where K. = 154 at 298 K: 2NO(g) + Br2(g) = 2NOBr(g) A reaction mixture was found to contain 4.48 102 moles of NO(g), 3.92x102 moles of Brg(e) and 7.91x102 moles of NOBr(g), in a 1.00 Liter container Indicate True (I) or False (E) for each of the following: 1. In order to reach equilibrium NOBr(e) must be consumed, 2. In order to reach equilibrium Ke must increase 3. In order to reach equilibrium NO must...
Consider the following reaction where K. = 154 at 298 K. 2NO(g) + Br2(g) + 2NOBr(8) A reaction mixture was found to...
Consider the following reaction where K. = 154 at 298 K. 2NO(g) + Br2(g) + 2NOBr(8) A reaction mixture was found to contain 4.66x10-2 moles of NO(g), 4.26x102 moles of Br2(g) and 9.65x102 moles of NOBr(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the...
Consider the following reaction where K. = 154 at 298 K: 2NO(g) + Br2(g) = 2NOBr(g)...
Consider the following reaction where K. = 154 at 298 K: 2NO(g) + Br2(g) = 2NOBr(g) A reaction mixture was found to contain 2.86x10-2 moles of NO(g), 3.93x10-2 moles of Br2(g) and 8.83x10-2 moles of NOBr(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium NOBr(g) must be consumed. 2. In order to reach equilibrium K, must increase. 3. In order to reach equilibrium NO must be...
Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give...
Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give the following information (298.15 K) NO (g) +1/2Br2(g) NOBr(g) Ke 4.5 2 NO (g)N2(g) 02(g) Ke 3.0 x 102 5. For the BrCl decomposition reaction 2BrCl(g) Br2(g Cl2(g) Initially, the vessel is charged at 500 K with BrCl at a partial pressure of 0.500 atm. At equilibrium, the partial pressure of BrC is 0.040 atm. Calculate Kp value at 500K
Consider the...
What is the equilibrium pressure At 373 K, Kp=0.416 for the equilibrium 2NOBr(g)?2NO(g)+Br2(g) If the pressures...
What is the equilibrium pressure At 373 K, Kp=0.416 for the equilibrium 2NOBr(g)?2NO(g)+Br2(g) If the pressures of NOBr(g) and NO(g) are equal, what is the equilibrium pressure of Br2(g)?
Consider the following reaction where K. = 154 at 298 K: 2NO(g) + Br2(g) = 2NOBr(g) A reaction mixture was found to contain 4.48 102 moles of NO(g), 3.92x102 moles of Brg(e) and 7.91x102 moles of NOBr(g), in a 1.00 Liter container Indicate True (I) or False (E) for each of the following: 1. In order to reach equilibrium NOBr(e) must be consumed, 2. In order to reach equilibrium Ke must increase 3. In order to reach equilibrium NO must...
Consider the following reaction where K. = 154 at 298 K. 2NO(g) + Br2(g) + 2NOBr(8) A reaction mixture was found to contain 4.66x10-2 moles of NO(g), 4.26x102 moles of Br2(g) and 9.65x102 moles of NOBr(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the...
Consider the following reaction where K. = 154 at 298 K: 2NO(g) + Br2(g) = 2NOBr(g) A reaction mixture was found to contain 2.86x10-2 moles of NO(g), 3.93x10-2 moles of Br2(g) and 8.83x10-2 moles of NOBr(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium NOBr(g) must be consumed. 2. In order to reach equilibrium K, must increase. 3. In order to reach equilibrium NO must be...
Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give the following information (298.15 K) NO (g) +1/2Br2(g) NOBr(g) Ke 4.5 2 NO (g)N2(g) 02(g) Ke 3.0 x 102 5. For the BrCl decomposition reaction 2BrCl(g) Br2(g Cl2(g) Initially, the vessel is charged at 500 K with BrCl at a partial pressure of 0.500 atm. At equilibrium, the partial pressure of BrC is 0.040 atm. Calculate Kp value at 500K
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