The numerical value of the equilibrium constant,
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- Le Chatelier’s principle states that “If you stress a system at equilibrium, the system will react to relieve the stress and return to equilibrium”. The following equation represents a chemical reaction at equilibrium: 2A (g) + 3B (g) <===> 2C (g) + 4D (g) ∆H = -378 kcal/mol (g) means gas In each case below, explain how the system reacts (forward direction, reverse direction or no change): The concentration of A is increased Heat is added to the system B is removed from the reaction Pressure is added The concentration of C is increasedarrow_forward1:18 Question 1 of 16 Consider the following chemical reaction at equilibrium: 2NO₂(g) = N₂O4(9) A) reactants If the container's volume is increased by a factor of 2, in which direction will the equilibrium shift? B) product Submit C) neither the reactants nor the product Tap here or pull up for additional resourcesarrow_forward7. 2CO2 (g) 200(g) + O2 (g). It was found that at 20 OC, the total pressure at equilibrium is 2.9 atm and that of CO2 is 0.8 atm. Calculate K. (Answer 2.14)arrow_forward
- (#30) The Equilibrium Constant and the "ICE Chart" Phosphorus pentachloride gas is formed according to the reaction by adding chlorine gas to phosphorus trichloride gas. Then the reaction reaches equilibrium. The equilibrium constant, Kc, equals 49.0 at 230°C. If 0.500 mole each of the reactants are added to a 5-L container, what is the equilibrium composition at 230°C? (30a) In blank #1, type-in our answer for the concentration of phosphorus pentachloride in the product at equilibrium. The unit is Molarity, but enter only the value of your answer with two decimal places. (30b) In blank #2, type in your answer for the concentration of phosphorus trichloride at equilibrium with two decimal places. (30c) In blank #3, type in your answer for the concentration of chlorine gas at equilibrium with two decimal places.arrow_forwardConsider the following system at equilibrium: P4 (g) + 6 H2 (g) = 4 PH3 (g) ΔΗ 110. 5 kJ If the volume was increased, what changes would have to occur to reestablish equilibrium? Select 2 correct answer(s) The reaction would shift right. The concentration of PH3 would increase. The concentration of P4 would increase The reaction would shift left. The concentration of H2 would decrease.arrow_forwardState the direction (forward or backward) in which each of the following equilibrium systems would be shifted upon the application of the stress listed beside the equation. (20 points) N,O, 2NOBr increase pressure add a + catalyst add Fe (s) remove CO, increase pressure decrease pressure increase NO, decrease H, decrease temperature increase temperature 2NO, 2NO 01. 02. 03. 04. 05. 06. 3Fe (s) + 4H,0 СаCо, (s) SnO.(s) + 2CO CO + Br. ++ Fe,O. + 4H, Cao (s) + CO, Sn(s) + 20O, CO, 2NO, 2NH, + H,O + Ha 07. 08. 09. 10. 2NO + O, N; C (s) 2S0. + O, 3H, CO: + heat 2C0 heat 2SO, ...arrow_forward
- 15.17 When the following reactions come to equilibrium, does the equilibrium mixture contain mostly reactants or mostly products? Kc = 1.5 × 10-10 (b) 2 SO2(8) + O2(8) = 2 S03(g) K,= 2.5 x 10° (a) N2(8) + O2(8) = 2 NO(g) %3Darrow_forward6. What is the correct equilibrium constant (K.) expression for the following reactions? (4 points) 2SO2(g) + O2(g) 2SO3(g) 4Cu(s) + O2(g) 2Cu2O(s)arrow_forward6. 0.300 mole of dinitogen tetraoxide was added to a 2.00 Litre flask. What is the equilibrium concentration of both gases? N2O4 (g) 5 2 NO2 (g) Keg = 4.50arrow_forward
- (10b) The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600K. COCl2(g) CO(g) + Cl2(g)If an equilibrium mixture of the three gases in a 11.8 L container at 600K contains 0.303 mol of COCl2(g) and 0.320 mol of CO, the equilibrium concentration of Cl2 is M. (25a) The equilibrium constant, K, for the following reaction is 1.75×10-2 at 609 K.COCl2 (g) CO (g) + Cl2 (g) An equilibrium mixture of the three gases in a 14.0 L container at 609 K contains 0.209 M COCl2, 6.04×10-2 M CO and 6.04×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 5.82 L? [COCl2] = M [CO] = M [Cl2] = Marrow_forwardConsider the endothermic reactionC (s) + H2O (g) ⇄ CO (g) + H2 (g)If the system is allowed to reach equilibrium, which direction will it shift if the following stresses are applied? (11a) Increase volume (11b) Decrease temperaturearrow_forwardConsider the following equilibria: (1) SO3(g) SO2(g) + 1/2O₂(g) (2) 2NO3(g) 2NO2(g) + O₂(g) Calculate the equilibrium constant for the reaction (3) SO₂(g) + NO3(g) SO3(g) + NO₂(g) O 1.6 x 10-4 O 1.3 x 10-² O 78 O 6.1 x 103 Kc = 4.8 x 10-4 Kc 1.4 x 10-3 = Kc = ???arrow_forward
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