Question

A) Part 1 For the reaction 3H2(g) + N2(g) → 2NH3(g) at 225 °C, the equilibrium constant is 1.7×10^2. If the equilibrium mixture contains 0.20 M H2 and 0.022 M N2, what is the molar concentration of NH3? Express your answer to two significant figures and include the appropriate units. [NH3] = B) Part 1 What is the Kc for the following equilibrium at 1000 °C? CO(g) + 3H2(g) → CH4(g) + H2O(g) [H2] = 0.20 M, [CO] = 0.40 M, [CH4] = 2.0 M, and [H2O] = 2.2 M ? Express your answer using two significant figures. Kc = C) Part 2 Consider the following reaction: PCl5(g) → PCl3(g) + Cl2(g) Part A Select the equilibrium constant expression for the reaction. Kc = [PCl5][PCl3][Cl2] Kc = [PCl3][Cl2][PCl5] Kc = [PCl5][PCl3] Part B Initially, 0.62 mol of PCl5 is placed in a 1.0 L flask. At equilibrium, there is 0.13 mol of PCl3 in the flask. What is the equilibrium concentration of PCl5? Express your answer to two significant figures and include the appropriate units. [PCl5] = Part C What is the equilibrium concentration of Cl2? Express your answer to two significant figures and include the appropriate units. [Cl2] = Part D What is the numerical value of the equilibrium constant, Kc, for the reaction? Express your answer using two significant figures. Kc = Part E If 0.15 mol of Cl2 is added to the equilibrium mixture, will the concentration of PCl5 increase or decrease? the concentration of PCl5 will increase the concentration of PCl5 will decrease

          A) Part 1
For the reaction
3H2(g) + N2(g) → 2NH3(g)
at 225 °C, the equilibrium constant is 1.7×10^2. If the equilibrium
mixture contains 0.20 M H2 and 0.022 M N2, what
is the molar concentration of NH3?
Express your answer to two significant figures and include the
appropriate units.
[NH3] = 

B) Part 1
What is the Kc for the following equilibrium at
1000 °C?
CO(g) + 3H2(g) → CH4(g) + H2O(g)
[H2] = 0.20 M, [CO] = 0.40 M, [CH4] = 2.0 M, and [H2O] = 2.2 M
?
Express your answer using two significant figures.
Kc = 

C) Part 2
Consider the following reaction:
PCl5(g) → PCl3(g) + Cl2(g)

Part A
Select the equilibrium constant expression for the reaction.
Kc = [PCl5][PCl3][Cl2]
Kc = [PCl3][Cl2][PCl5]
Kc = [PCl5][PCl3]

Part B
Initially, 0.62 mol of PCl5 is placed in a 1.0 L flask. At
equilibrium, there is 0.13 mol of PCl3 in the flask. What is the
equilibrium concentration of PCl5?
Express your answer to two significant figures and include the
appropriate units.
[PCl5] = 

Part C
What is the equilibrium concentration of Cl2?
Express your answer to two significant figures and include the
appropriate units.
[Cl2] = 

Part D
What is the numerical value of the equilibrium constant,
Kc, for the reaction?
Express your answer using two significant figures.
Kc = 

Part E
If 0.15 mol of Cl2 is added to the equilibrium mixture, will the
concentration of PCl5 increase or decrease?
the concentration of PCl5 will increase
the concentration of PCl5 will decrease

Added by Jose Luis F.

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