At 35°C, K = 1.9 × 10-5 for the reaction 2 NOCI(g) = 2 NO(g) + Cl2 (9) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.2 moles of pure NOC1 in a 2.0-L flask [NOCI] M [NO] = M [Cl2] = M b. 1.0 mole of NOC1 and 1.0 mole of NO in a 1.0-L flask [NOCI] |M [NO] M [Cl2] = M c. 2.8 mole of NOC1 and 1.0 mole of Cl2 in a 1.0-L flask [NOCI] M [NO] = M [Cl2] = M

At 35°C, K = 1.9 × 10-5 for the reaction 2 NOCI(g) = 2 NO(g) + Cl2 (9) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.2 moles of pure NOC1 in a 2.0-L flask [NOCI] M [NO] = M [Cl2] = M b. 1.0 mole of NOC1 and 1.0 mole of NO in a 1.0-L flask [NOCI] |M [NO] M [Cl2] = M c. 2.8 mole of NOC1 and 1.0 mole of Cl2 in a 1.0-L flask [NOCI] M [NO] = M [Cl2] = M

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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For the following reaction, Kc CO (g) + Cl₂ (g) = COCI₂(g) A reaction mixture initially contains a CO concentration of 0.1510 M and a Cl2 concentration of 0.175 M at 1000 K. What is the equilibrium concentration of COCl2 at 1000 K? = 255 at 1000 K.
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K = 1.5 x 10-5 for the reaction 2 NOCI(9) = 2 NO(9) + Cl2 (9) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 3.2 moles of pure NOCI in a 2.0-L flask [NOCI] =| M [NO] = | M (CL] = M b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask [NOCI] = M [NO] =| M [Cl2] = [ M c. 3.2 mole of NOCI and 1.0 mole of Cl, in a 1.0-L flask [NOCI] = [ M [NO] = [ M
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