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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At a particular temperature, Kp = 0.230 for the reaction N2O4(g) 2NO2(g) 1a) A flask containing only N2O4(g) at an initial pressure of 3.40 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium. 1b) With no change in the amount of material in the flask, the volume of the container in question is decreased to 0.300 times the original volume. Assuming constant temperature, calculate the (new) total pressure, at equilibrium.
For the following hypothetical equilibrium at 25°C, what is the value of the equilibrium constant; Kp if the concentrations at equilibrium are as shown? {calculate K, then convert to K,} A+ 2BSC [A] = 4.5 x 10-5 M [B] = 2.2 x10-2 M [C] = 9.4 x 10-3 M а. 1.76 х 104 с. 4.3 х 105 b. 1.05 х 107 d. 7.18 x 102
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.
The equilibrium constant Kp for the reaction CCl4(g) —> C(s) + 2Cl2(g) at 700˚C is 0.76. Determine the initial pressure of carbon tetrachloride that will produce an equilibrium pressure of 1.5 atm for Cl2 at 700˚C. (Since C is a solid it can be left out of the ICE chart.)
The equilibrium constant, Kp, for the reaction PCl5 (g) > PCl3 + Cl2 is 1.26 at 250°C. The reaction is started with PCl5, PCl3, and Cl2 at 0.01, 0.2 and 0.5 atm at 250°C. When will the reaction come to equilibrium?
A pure sample of SO3 is placed in a container and reacts according to the equation 2 SO3(g) ⇄ 2 SO2(g) + O2(g) Kp = 4.00At equilibrium the partial pressure of O2 is 0.10 atm. Calculate the pressure of SO3 remaining at equilibrium.
Hydrogen iodide can decompose into hydrogen and iodine gases. 2 HI(g) --> H2(g) + I2(g) Kp = 0.0180 If 0.05 atm is sealed in flask initially, what is the partial pressure of I2(g) at equilibrium?
At a given temperature, an equilibrium mixture associated with the reaction A(g) + 2 B(g) = 2 C(g) contains: [A] = 0.0250 M [B] = 0.150 M [C] = 0.550 M What is the value of K, for this reaction at the same temperature?
At 1560 oC the equilibrium constant for the reaction: 2 IBr(g) I2(g) + Br2(g) is KP = 0.846. If the initial pressure of IBr is 0.00674 atm, what are the equilibrium partial pressures of IBr, I2, and Br2?p(IBr) = p(I2) = p(Br2) =
14.25 Consider the following reaction at 1600°C. Br2(g) = 2Br(g) When 1.05 moles of Br, are put in a 0.980-L flask, 1.20 percent of the Br, undergoes dissociation. Calculate the equilibrium constant K. for the reaction.
The formation of hydrogen sulfide at 300°C. Ca(HCO3)2 (s) → H2O (g) + CO2 (g) + CaCO3 (s) KP = 2.88 If a 26 gram sample of Ca(HCO3 is put into a 28.6 L container and heated to 300°C, what percent of the H2O will be produced at equilibrium?
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

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