Solve the following problems.
1) A solution is prepared by dissolving 2.15 g of sulfur (S8) in 105.0 g of acetic acid (HC2H3O2). What is the freezing point of the solution?
The freezing point of the solution is _______________ oC.
|
Freezing point of pure acetic acid: |
16.60 oC |
|
Kf of acetic acid |
3.59 oC/m |
2) An aqueous solution of citric acid (H3C6H5O7) has a concentration of 0.750 m. If the density of the solution is 1.100 g/mL, what is the molar concentration of the solution?
The molar concentration of the solution is ___________________ M.
3) Consider the following equilibrium:
N2O4(g) <--> 2NO2(g) ; Kc = 0.125
If you put 0.500 moles of N2O4 in a 10.00 L reaction flask, how many moles of NO2 will be produced at equilibrium? Hint: I am not asking for the concentration of NO 2 as your answer, but you will have to find the concentration to solve the problem. You may need the quadratic formula to solve this problem.
_____________ moles of NO2 gas are produced at equilibrium.
4) Consider the following equilibrium:
COCl2(g) <--> CO(g) + Cl2(g) ; Kc = 8.05x10-4
You have a vessel filled with 1.50 M COCl2, 0.00050 M CO, and 0.00025 M Cl2. Is the reaction at equilibrium? If it is not, will the reaction proceed to form more products or more reactants?
The reaction ______________ (is/is not) at equilibrium.
The reaction will proceed to produce more _______________ (products/reactants). Answer this one only if the reaction is not at equilibrium!
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