At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, K.3 A(g) + 2 B(g) =4 C(g)K = 2.13 x 10If, at this temperature, 1.50 mol of A and 3.80 mol of B are placed in a 1.00 L container, what are the concentrations of A. B,and C at equilibrium?[A] =[B] =(C) =M

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Answered: At a certain temperature, this reaction…

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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The equilibrium constant, K, for the following reaction is 1.80×10-² at 698 K. 2HI(g) H₂(g) + I₂(g) If an equilibrium mixture of the three gases in a 19.0 L container at 698 K contains 0.230 mol of HI(g) and 0.345 mol of H₂, the equilibrium concentration of 12 is M.
The equilibrium expression for the the reaction:H2(g) + I2(g) <--> 2HI(g) would be: Given the reaction: A + B <--> C + DThe concentrations at equilibrium are [A] = 1 M, [B] = 1 M, [C] = 2 M, and [D] = 2 M. What is the value of the equilibrium constant (K)?
please explain and give complete answer
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At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g)↽−−⇀4C(g) ?c=2.13×10^25 If, at this temperature, 2.30mol of A and 3.60mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A]= M [B]= M [C]= M
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A student ran the following reaction in the laboratory at 735 K: N2(g) + 3H2(g) = 2NH3(g) When she introduced 0.0402 moles of N2 (g) and 0.0547 moles of H2(g) into a 1.00 liter container, she found the equilibrium concentration of NH3 (g) to be 0.000861 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Кс =

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