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?

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Chapter1: Chemical Foundations
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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
Transcribed Image Text: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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