A sealed chamber contains an equilibrium mixture of NO₂(g) and N₂O4(g) at 300°C.The partial pressures of NO₂ and N₂O4 are 1.8 and 24.latm, respectively. What isthe value of K, for the dimerization of NO: 2 NO₂(g)N₂O4(g) at 300°C?a) 0.40 b) 1.1 c) 2.5 d) 4.0 e) 7.4 t) 59.3 g) 16.6 h) 23.1

Answer: Kb = 7.4 So, the correct option is (e) Explanation:

Answered: A sealed chamber contains an…

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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Calculate the concentrations of all species at equilibrium. Calculate the Kp for this reaction at 25.0°C Given that the reaction quotient for this equilibrium is 5.4 mol/L. SO2(g) + Cl2(g) <---> SO2Cl2(g) Kc= 0.364 A 2.50 L container initially contains 0.252 moles of sulfur dioxide, 0.750 moles of CHlorine Gas, and 0.850 moles of sulfuryl chloride.
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4. IBr decomposes according to the reaction at 150 C: 2 IB (g) = 12 (g) + Brz (g) If IBr is placed in a container at an initial pressure of 5.0 atm, what will be its equilibrium pressure at 150°C? K = 8.3 x 10-3
Consider the equilibrium system involving the decomposition of nitrogen monoxide. 2NO(g) N2(g) + O2(g) K = [N2] [O2] = 0.243 at 279 K [NO]2 A flask originally contains 0.345 M nitrogen monoxide. Calculate the equilibrium concentrations of the three gases. [NO] = M [N2] = M [O2] = M

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