II. GENERAL INSTRUCTIONSRead and analyze carefully each problem. Show your complete solution.1. At 500 K, the following concentrations were measured: [N2] =3.0 x 102 M [Hz]= 3.7 x 102 M, (NH3) = 16 x 10-2² M2NH3(g)N2(g) + 3H2(g)a What is the equilibrium constant expression?b. What is the equilibrium constant?2 N2(g) + 3H2(g) 2NH3(g)At 375°C, the equilibrium constant of the reaction is 2 79 x 10-5a. What is Kp?b. What is the partial pressure of NHS if the partial pressures of H₂ and Nz are1.24 atm and 2.17 atm, respectively?3. Consider the following reaction where Kc = 3900 at 2000 K2SO2 (g) + O2(g) = 250³(g)4a Write the equilibrium constant expression

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refully each problem. Show your complete solution. 1. At 500 K, the following concentrations were measured [N₂] =3.0 x 10-² M, [Hz] = 3.7 x 102 M, (NH3) = 1.6 x 10-² M 2NH3(g) N2(g) + 3H2(g) a What is the equilibrium constant expression? b. What is the equilibrium constant?

refully each problem. Show your complete solution. 1. At 500 K, the following concentrations were measured [N₂] =3.0 x 10-² M, [Hz] = 3.7 x 102 M, (NH3) = 1.6 x 10-² M 2NH3(g) N2(g) + 3H2(g) a What is the equilibrium constant expression? b. What is the equilibrium constant?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 2RQ: What is the law of mass action? Is it true that the value of K depends on the amounts of reactants...

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Applications of Molecular Spectroscopy

When light sources pass through the diffraction grating then light splits into different wavelengths. The light source produces two types of patterns that are shown as destructive and non-destructive. The light source is in the form of quanta that is quantitation.

Question

II. GENERAL INSTRUCTIONS
Read and analyze carefully each problem. Show your complete solution.
1. At 500 K, the following concentrations were measured: [N2] =3.0 x 102 M [Hz]
= 3.7 x 102 M, (NH3) = 16 x 10-2² M
2NH3(g)
N2(g) + 3H2(g)
a What is the equilibrium constant expression?
b. What is the equilibrium constant?
2 N2(g) + 3H2(g) 2NH3(g)
At 375°C, the equilibrium constant of the reaction is 2 79 x 10-5
a. What is Kp?
b. What is the partial pressure of NHS if the partial pressures of H₂ and Nz are
1.24 atm and 2.17 atm, respectively?
3. Consider the following reaction where Kc = 3900 at 2000 K
2SO2 (g) + O2(g) = 250³(g)
4
a Write the equilibrium constant expression

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