A.) Some NOBr is placed in a flask and heated to 358 K. When equilibrium is reached, the flask is found to contain NOBr (2.43×102 M), NO (2.16×10-2 M), and Br2 (2.05×10-2 M). What is the value of the equilibrium constant for the following at reaction at 358 K?2NOBr(g) 2NO(g) + Br2(g) K = B.) A mixture of H2 and I2 is allowed to react at 699 K. H2(g) + I2(g) 2HI(g)The initial concentration of the reactants are [H2] = 0.2100 M and [I2] = 0.2380 M. After the system reaches equilibrium, it is found that the I2 concentration has decreased to 0.0628 M. Based on these data, determine the value of the equilibrium constant, K, for this reaction.K =

(A) Consider the given information is as follows; Equilibrium concentration of NOBr=NOBr=2.43×102…

Answered: A.) Some NOBr is placed in a flask and…

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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A.) Some NOBr is placed in a flask and heated to 358 K. When equilibrium is reached, the flask is found to contain NOBr (2.43×10² M), NO (2.16×10^-2 M), and Br₂ (2.05×10^-2 M). What is the value of the equilibrium constant for the following at reaction at 358 K?

2NOBr(g) 2NO(g) + Br₂(g) K =

B.) A mixture of H₂ and I₂ is allowed to react at 699 K. H₂(g) + I₂(g) 2HI(g)
The initial concentration of the reactants are [H₂] = 0.2100 M and [I₂] = 0.2380 M. After the system reaches equilibrium, it is found that the I₂ concentration has decreased to 0.0628 M. Based on these data, determine the value of the equilibrium constant, K, for this reaction.
K =