Answered: The equilibrium constant for the…

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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Question

The equilibrium constant for the reaction below is K_p=2.26×10^–3 at a certain temperature. A container is pressurized until the pressure of NO is 0.400 atm and the pressure of Br₂ is 0.250 atm.

2 NO (g) + Br₂ (g) ⇄ 2 NOBr (g)

Calculate the equilibrium pressure of NOBr in the container by the method of approximation as discussed in class. Note: Entering the exact answer, solved with a graphing calculator, will not receive credit. Approximate the answer.

P_NOBr= atm (Answer with 3 significant figures)

Expert Solution

Step 1

$\begin{array}{rcl} G i v e n d a t a, \\ K p & = & 2.26 \times 10^{- 3} \\ I n i t i a l p r e s s u r e o f N O & = & 0.400 a t m \\ I n i t i a l p r e s s u r e o f B r_{2} & = & 0.250 a t m \end{array}$

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