chemistry lab
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Worksheet 10 Equilibrium and Acids/Bases Lab: 1 2 3 MCU SPRING 2015
1. Write an appropriate equilibrium expression for the following unbalanced chemical equations that have achieved equilibrium
2. Gaseous phosphorus pentachloride decomposes according to the unbalanced equation: PCl5 (g) ⬄ PCl3 (g) + Cl2 (g)
The equilibrium system at 100 °C shows the concentrations of all substances to be [PCl5] = 1.10 x 10-2 M, [PCl3] = 0.325 M, and [Cl2] = 3.95 x 10-3 M. Calculate the value of Kc for the reaction and evaluate whether the reactant or product side is favored at equilibrium.
SO2 (g) + O2 (g) ⬄ SO3 (g) CH4 (g) + H2O (l) ó H2 (g) + CO (g) Balanced equation Balanced equation
Equilibrium expression Equilibrium expression
FeO (s) + H2 (g) ⬄ Fe (s) + H2O (l) Cu(OH)2 (s) ⬄ Cu2+ (aq) + OH- (aq) Balanced equation Balanced equation
Equilibrium expression Equilibrium expression
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3. The synthesis of ammonia, NH3, can be described by the following unbalanced equation: N2 (g) + H2 (g) ⬄ NH3 (g)
For the reaction described above done at 500 °C, the equilibrium concentrations was determined to be as follows: [N2] = 0.921 M, [H2] = 0.763 M, [NH3] = 0.157 M. Based on these values, calculate the equilibrium constant, Kc, at 500 °C. Evaluate the equilibrium as favoring the reactant or product side.
4. The equilibrium constant, Kc, for the unbalanced reaction H2 (g) + F2 (g) ⬄ HF (g)
has a value of 2.10 x 104 at a particular temperature. When the system is analyzed at equilibrium at this temperature, the concentrations of both H2 (g) and F2 (g) are found to be 8.10 x 10-3 M. Based on this information what would be the equilibrium concentration of HF(g) under these conditions.
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5. For the reaction as described by the unbalanced equation: H2O (g) ⬄ H2 (g) + O2 (g)
Kc = 2.40 x 10-3 at 55.0 °C. Upon reaching equilibrium it is found that the [H2] = 1.10 x 10-1 M and [O2] = 1.95 x 10-2 M. What would be the equilibrium concentration of H2O (g) at this temperature?
6. Suppose the reaction system UO2 (s) + 4HF (g) ⬄ UF4 (g) + 2H2O (l)
has reached a state of equilibrium within a reaction flask. Predict the effect of each of the following changes to the position of the equilibrium. Indicate whether the equilibrium will shift with more forward reaction (favoring more products formed), shift towards more reverse reaction (favoring more reactants reformed), or produce no shift in equilibrium
Change in reaction condition Equilibrium Shift Expected
a. Moles of reactants are doubled
b. Additional UF4 (g) is added to the reaction flask
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7. Write the equilibrium equation for the dissociation and the expression for the solubility product constant, Ksp, for the following compounds
a) Copper (II) sulfide, CuS
b) Lead (II) fluoride, PbF2
c) Iron (III) hydroxide, Fe(OH)3
8. Calculate the solubility product constant, Ksp, for a saturated solution of the following partially soluble ionic compounds with the indicated ion concentrations.
a) Copper (I) chloride, CuCl, where [Cu+] = 1.10 x 10-3 M and [Cl-] = 1.10 x 10-3 M
c. Water is removed from the reaction
d. A metal catalyst is added to the reaction
e. Moles of reactants are halved
f. The reactants are cooled to half its current temperature
g. The products are heated as a hotplate is turned on
h. UF4(g) is vacuumed out as it forms in the reaction
i. Additional UO2 (s) is added to the reaction flask
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b) Silver chromate, Ag2CrO4, where [Ag+] = 1.30 x 10-4 M and [CrO42-] = 6.50 x 10-5 M
9. Given their Ksp value, calculate the molar solubility, S, of each ion of the following ionic compounds in solution
a) Manganese (II) sulfide, MnS Ksp = 2.50 x 10-10
b) Lead (II) carbonate, PbCO3 Ksp = 7.40 x 10-14
c) Calcium hydroxide, Ca(OH)2 Ksp = 6.50 x 10-6
d) Silver sulfate, Ag2SO4 Ksp = 1.20 x 10-5