# Equilibrium Practice Worksheet #1

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"Equilibrium Practice Worksheet #1"

```					                   Equilibrium Practice Worksheet #1
Solve the following problems using the ICE method.

1. Carbonyl bromide, COBr2, decomposes to CO and Br2 at 73ºC. If you begin
with 0.10 moles of COBr2 in a 2.5 Liter flask and find that there are 0.015
moles of COBr2 at equilibrium, calculate the equilibrium concentrations of the
products. What is K for this reaction? Is this reaction reactant-favored or
product-favored at equilibrium?
COBr2 (g)   º CO (g) + Br         2 (g)

2. Hydrogen fluoride gas can be formed from hydrogen and fluorine gases
according to the balanced equation shown below. At a specific temperature,
the equilibrium constant for this reaction is 37.6. What are the partial
pressures of all of the gases at equilibrium when the initial partial pressures of
hydrogen gas and fluorine gas are 0.600 atm?
H2 (g) + F2 (g)    º      2 HF (g)

3. Cyclohexane, C6H12, can isomerize (change into a compound of the same
formula but different structure) to form methylcyclopentane, C5H9CH3. The
equilibrium constant is 0.12 at 25ºC. If the initial concentration of cyclohexane
is 0.016 M, what are the concentrations of each gas at equilibrium?
C6H12 (g)   º C H CH
5   9       3   (g)

4. Nitrogen gas reacts with oxygen gas at high temperature to make nitrogen
oxides. This is a major source of air pollution from auto exhaust. At 1500 K,
the equilibrium constant for the formation of nitrogen monoxide from its
elements is 1.0 x 10-5. Calculate the equilibrium concentration of NO when the
initial concentration of N2 is 0.60 M and O2 is 0.30 M.
N2(g) + O2(g)   º       2 NO(g)

5. The equilibrium constant, Kc, for the following reaction is 5.9 x 10-3 at 250ºC.
Suppose 0.17 moles of N2O4(g) is placed in a 5.00 L flask. What is the
equilibrium concentration of NO2(g)? Note: solve for x using the
approximation method and then check to see if it is a valid approximation.
N2O4(g)   º 2 NO (g) 2

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