A student ran the following reaction in the laboratory at 617 K: Co(g) + Cl2(g) = cocl2(g) When she introduced 0.156 moles of CO(g) and 0.185 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCI2(g) to be 0.117 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. K. =

A student ran the following reaction in the laboratory at 617 K: Co(g) + Cl2(g) = cocl2(g) When she introduced 0.156 moles of CO(g) and 0.185 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCI2(g) to be 0.117 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. K. =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Methanol liquid burns readily in air. One way to represent this equilibrium is: CH₂OH(1) + 3/2 0₂(g) CO₂(g) + 2 H₂O(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) 2 CH₂OH(1) + 3 O₂(g) 2) 2 CO₂(g) + 4H₂O(g) 2 CO₂(g) + 4H₂O(g) 2 CH₂OH(1) + 3 O₂(g) CH₂OH(1) + 3/2 0₂(g) K3 K₁ = K₂ = 3) CO₂(g) + 2 H₂O(g) Drag and drop your selection from the following list to complete the answer: K² (1/K)² 1/K
Suppose a 250. mL flask is filled with 0.60 mol of Br₂, 1.9 mol of BrOCI and 1.3 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrC1 (g) The equilibrium constant K for this reaction is 1.98 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.
Nitrosyl chloride, NOCI, decomposes to NO and Cl, at high temperatures: 2NOCI(g) -> 2NO(g) + Cl2(g) Suppose you place 2.00 mol NOCI in a 1.00-L flask and raise the temperature to 462°C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.
A student ran the following reaction in the laboratory at 545 K: COC12 (g) CO(g) + Cl₂ (g) When she introduced 0.604 moles of COC12 (g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂ (g) to be 0.0302 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
Please answer with the correct number of significant digits. At a certain temperature, the equilibrium constant K for the following reaction is 9.7 x 10¹¹: NO₂(g) + CO(g) NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 42. L reaction vessel is filled with 1.2 mol of NO₂ and 1.2 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. NO(g) + CO₂(9) 1 NO₂(9)+CO (9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 NO₂(9)+2CO(g) 1 2 NO(g) +2C0₂(9) There will be very little NO₂ and CO. There will be very little NO and CO₂. Neither of the above is true. K-O K-0 X
A student ran the following reaction in the laboratory at 600 K: CO(g) + Cl₂(g) —COCI₂(g) When he introduced CO(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.09 atm and the initial partial pressure of Cl₂ was 1.22 atm, he found that the equilibrium partial pressure of Cl₂ was 0.405 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр
A student ran the following reaction in the laboratory at 290 K:2CH2Cl2(g) CH4(g) + CCl4(g) When she introduced 8.37×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CH2Cl2(g) to be 6.14×10-3M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
Part A The equilibrium constant, Kc, for the decomposition of COC2 to CO and Cl2 is 0.68. If an equilibrium mixture contains 0.38 M CÓ and 0.55 M Cl2, what is the molar concentration of COCl2 ? COC2 (g) = CO(g) + Cl2 (g) Express your answer to two significant figures and include the appropriate units.
5. The reaction: 2NO₂(g) + 7H₂(g) = 2NH3(g) + 4H₂O(g) was allowed to reach equilibrium at 455 K. Analysis showed that there was 34.6 g of NO2, 53.2 g of H₂, 52.6 g of NH3 and 87.4 g H₂O present in a 2.65 L vessel once equilibrium was achieved. a. Determine the equilibrium concentration for both reactants. b. Determine the equilibrium concentration for both products. C. Write the Kc expression. d. Solve for the Kc. e. Solve for the Kp at the same temperature.
Consider the following reaction where K. = 10.5 at 350 K: 2 CH;Cl2 (g)=CH4 (g)+ CCI4 (g) A reaction mixture was found to contain 1.10x10-2 moles of CH,Cl, (g), 4.63×10-2 moles of CH4 (g), and 3.70×10² moles of CCl (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: v 1. In order to reach equilibrium CH,Cl,(g) must be produced. v 2. In order to reach equilibrium K, must decrease v 3. In order to reach equilibrium CH, must be consumed. v 4. Qc is greater than K. 5. The reaction is at equilibrium. No further reaction will occur. T
A student ran the following reaction in the laboratory at 316 K:2CH2Cl2(g) CH4(g) + CCl4(g)When he introduced CH2Cl2(g) at a pressure of 0.487 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CCl4(g) to be 0.219 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction.
Suppose a 500. mL flask is filled with 0.30 mol of Br₂, 1.2 mol of OC1, and 0.60 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂ (g) BrOCI(g) + BrCl(g) The equilibrium constant K for this reaction is 4.09 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places.