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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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For the reaction below, you start with 3.00 atm of NO(g) and 2.00 atm of Br₂(g) and no NOBr(g) in a closed container at a temperature of 298 K. At equilibrium the total pressure in the container is 3.60 atm. What is the Kp for this reaction at 298 K? 2 NO(g) + Br₂(g) ⇌ 2 NOBr(g)
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- The following reaction was initiated with NOCl(g), with a partial pressure of NOCl(g) = 0.66 atm. The reaction achieved equilibrium at 25⁰C where equilibrium partial pressure for NOCl(g) : (?????(?) ) = 0.33 atm. Calculate the KC value for this reaction. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) A) 3.3 × 10-4 B) 0.165 C) 3.3 D) 6.74 × 10-3 E) 0.0042 atmarrow_forwardAn equilibrium is established for the reaction 2 CO(g) + MoO₂(s) ⇌ 2 CO₂(g) + Mo(s). Use the expression for Kp from part a. If at equilibrium the partial pressure of carbon monoxide is 5.21 atm and the partial pressure of the carbon dioxide is 0.753 atm, then what is the value of Kp?arrow_forwardConsider the reaction. Br2(g)+Cl2(g)⇌2BrCl(g) Kp=1.11×10−4 at 150 K A reaction mixture initially contains a Br2 partial pressure of 755 torr and a Cl2 partial pressure of 735 torr at 150 K. Calculate the equilibrium partial pressure of BrCl.arrow_forward
- Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)arrow_forwardA reaction vessel is charged with 0.50 atm of A and 0.220 atm of B. Once the reaction reaches equilibrium, what is the equilibrium partial pressure of B? Kp for this reaction is 67.2 A (g) ⇌ 2 B (g)arrow_forwardCalculate the pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2 produced when a sample of NOCl with a pressure of 10.0 atm comes to equilibrium according to this reaction:2NOCl(g) ⇌ 2NO(g) + Cl2(g) KP = 4.0 × 10−4arrow_forward
- Consider the following reaction where K = 77.5 at 600 K. CO(g) + Cl₂(g) 2 CoCl₂(g) A reaction mixture was found to contain 1.89×10-² moles of CO(g), 4.43×10-² moles of Cl₂(g) and 0.106 moles of COCI₂(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 reverse direction to reach equilibrium. C. is at equilibrium.arrow_forwardFor the reaction PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) Kp = 1.45 × 10⁻⁴ at 160 °C. A 1.00 L vessel at 160 °C is filled with PCl₅(g) at an initial pressure of 4.00 atm and allowed to come to equilibrium. What will be the pressure (in atm) of Cl₂(g) at equilibrium?arrow_forwardFor the reaction PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) Kp = 1.45 × 10⁻⁴ at 160 °C. A 1.00 L vessel at 160 °C is filled with PCl₅(g) at an initial pressure of 3.75 atm and allowed to come to equilibrium. What will be the pressure (in atm) of Cl₂(g) at equilibrium?arrow_forward
- Initially, 2.0 moles of N2(g) and 4.0 moles of H2(g) were added to a 1.0-liter container and the reaction below then occurred. The equilibrium concentration of NH3(g) = 0.55 M at 700.°C. The value for Kc at 700.°C for the formation of ammonia is: 3H2(g) + N2(g) ⇌ 2NH3(g) a) 1.0 x 10^-1 b) 5.5 x 10^-2 c) 5.5 x 10^-3 d) 3.0 x 10^-1 e) The correct answer was not initially availablearrow_forwardA sample of H2S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium. What is the total pressure of all gases in the container? 2H2S(g) ⇌ 2H2(g) + S2(g) Kp = 3.85 x 10-7 A sample of H2S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium. What is the total pressure of all gases in the container? 2H2S(g) ⇌ 2H2(g) + S2(g) Kp = 3.85 x 10-7 0.793 atm 0.387 atm 0.497 atm 0.215 atm 0.624 atmarrow_forwardAn empty steel container is filled with 4.6 atm of H₂ and 1.0 atm of F₂. The system is allowed to reach equilibrium according to the reaction below. If Kp = 0.45 for this reaction, what is the equilibrium partial pressure of HF? H₂ (g) + F₂ (g) ⇌ 2 HF (g)arrow_forward
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