The reaction\[ 2 \text{NO} (g) + \text{Br}_2 (g) \rightleftharpoons 2 \text{NOBr} (g) \]has \( K_p = 109 \) at 25°C. If the equilibrium partial pressure of \(\text{Br}_2\) is 0.0250 atm and the equilibrium partial pressure of \(\text{NOBr}\) is 0.0857 atm, calculate the partial pressure of \(\text{NO}\) at equilibrium.Partial pressure = \_\_\_\_ atm An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature by the reaction:\[ 3 \text{H}_2(\text{g}) + \text{N}_2(\text{g}) \rightleftharpoons 2 \text{NH}_3(\text{g}) \]At equilibrium, the concentrations are \([\text{H}_2] = 6.0 \, \text{M}\), \([\text{N}_2] = 12 \, \text{M}\), and \([\text{NH}_3] = 4.0 \, \text{M}\). What were the concentrations of nitrogen gas and hydrogen gas that were reacted initially?\[[\text{H}_2]_0 = \underline{\hspace{2cm}} \, \text{M}\]\[[\text{N}_2]_0 = \underline{\hspace{2cm}} \, \text{M}\]

Answered: The reaction 2NO(g) + Br₂ (g) — 2…

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 reaction

\[ 2 \text{NO} (g) + \text{Br}_2 (g) \rightleftharpoons 2 \text{NOBr} (g) \]

has \( K_p = 109 \) at 25°C. If the equilibrium partial pressure of \(\text{Br}_2\) is 0.0250 atm and the equilibrium partial pressure of \(\text{NOBr}\) is 0.0857 atm, calculate the partial pressure of \(\text{NO}\) at equilibrium.

Partial pressure = \_\_\_\_ atm

An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature by the reaction:

\[ 3 \text{H}_2(\text{g}) + \text{N}_2(\text{g}) \rightleftharpoons 2 \text{NH}_3(\text{g}) \]

At equilibrium, the concentrations are \([\text{H}_2] = 6.0 \, \text{M}\), \([\text{N}_2] = 12 \, \text{M}\), and \([\text{NH}_3] = 4.0 \, \text{M}\). What were the concentrations of nitrogen gas and hydrogen gas that were reacted initially?

\[[\text{H}_2]_0 = \underline{\hspace{2cm}} \, \text{M}\]

\[[\text{N}_2]_0 = \underline{\hspace{2cm}} \, \text{M}\]

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This problem is based on stoichiometric calculation where all the reactant species react in the molar ratio of their stoichiometric coefficients and all the product species formed are also in the molar ratio of their stoichiometric coefficients.

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