1. The relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for a process is K = ____________.
2. Consider the following equilibrium.
2 SO2(g) + O2(g) 2 SO3(g)
From which of the following starting conditions would it be
impossible for this equilibrium to be achieved?
a. 0.25 mol SO2(g) and 0.25 mol O2(g) in a 1.0-L container
b. Equilibrium can be achieved from any of these starting conditions.
c. 0.75 mol SO2(g) in a 1.0-L container
d. 1.0 mol SO3(g) in a 1.0-L container.
e. 0.50 mol O2(g) and 0.50 mol SO3(g) in a 1.0-L container
3. The equilibrium constant for reaction (1) below is 4.22 x 10-3. The value of the equilibrium constant for reaction (2) is
(1) 3 A + 2 B 2 D + E
(2) 2 D + E 3 A + 2 B
a. 5.78 x 10-2
c. The value of K2 cannot be determined from the data given.
d. 1.78 x 10-5
e. 4.22 x 10-3
4. The equilibrium constant for reaction (1) is K. What is the equilibrium constant for equation (2)?
(1) SO2(g) + 1/2O2(g) SO3(g)
(2) 2SO3(g) 2SO2(g) + O2(g)
5. The equilibrium constant for reaction (1) is K. What is the equilibrium constant for equation (2)?
(1) (1/3)N2(g) + H2(g) (2/3)NH3(g)
(2) 2NH3(g) N2(g) + 3H2(g)
6. The concentration (mol/L) of a pure substance in its pure liquid or pure solid phase is given by _______.
a. (molar volume)(molecular weight)
b. (mass)(specific gravity)
c. density divided by molar mass
d (Avogadro's number)(specific volume)
e. molar mass divided by density
1.A - See
2. C - Because the existence of only SO2 do not suffice enough substance for the reaction to take ...
The solution provides detailed explanation for the problem.