Indicate the mass expression for the following reaction:
3Y_{2}(g) + X_{2}(g) ↔ 2XY_{3}
Determine the equilibrium constant for the system 2XY_{3} ↔ 2X + 3Y_{2} at 25°C. The concentrations are shown here: [XY_{3}] = 1.23 x 10^{-2} M, [X] = 2.50 x 10^{-2} M, [Y_{2}] = 3.75 x 10^{-2} M
2.18 x 10^{-4}
3.30 x 10^{-8}
7.19 x 10^{-3}
9.81 x 10^{-6}
None of these
One mole of gaseous HA is placed in a one liter container. At equilibrium it is 18% dissociated according to the equation shown here:
2HA ↔ 2H + A_{2}
Determine the equilibrium constant.
K = 0.82
K = 0.0071
K = 0.0043
K = 0.0094
K = 0.0012
You are given a box containing NH_{3}, N_{2}, and H_{2} at equilibrium at 1000°C. Analysis of the contents shows that the concentration of NH_{3} is 0.102 mole/liter, N_{2} is 1.03 moles/liter, and H_{2} is 1.62 moles/liter. Calculate K for the reaction: 2NH_{3}(g) ↔ N_{2}(g) + 3H_{2}(g)
2.37 x 10^{-3}
4.21 x 10^{2}
3.89 x 10^{-4}
3.89 x 10^{4}
9.02 x 10^{-6}
Consider the following equilibrium:
X_{2}(g) + Y_{2}(g) ↔ 2XY(g) + energy
Addition of XY(g) will:
Cause [X_{2}] to increase
Drive the reaction toward the right
Cause the energy of the system to increase
Cause [Y_{2}] to decrease
Two of these occur
Consider the following equilibrium:
X_{2}(g) + Y_{2}(g) ↔ 2XY(g) + energy
Heating the system will:
Cause [X_{2}] to decrease
Drive the reaction toward the right
Cause [Y_{2}] to decrease
Cause [XY] to decrease
Two of these occur
Which of the following is always true for a reaction whose value for K is 4.4 x 10^{4}?
The reaction proceeds far to the right
The reaction proceeds far to the left
The reaction occurs quickly
The reaction occurs slowly
Two of these
Imagine a one liter container into which 2.0 mol samples of gaseous substances A, B, and C are introduced. A and B react according to the following equation:
A(g) + B(g) ↔ 2C(g)
If the value of K = 4.2, in what direction does the equilibrium exist?
Far to the right
Slightly to the right
Far to the left
Slightly to the left
The reaction is at equilibrium
Imagine a one liter container into which 2.0 mol samples of gaseous substances A, B, and C are introduced. A and B react according to the following equation:
A(g) + B(g) ↔ 2C(g)
If K = 2.68 for this reaction, what is the equilibrium concentration of C?
2.02 M
1.3 M
2.7 M
0.7 M
None of these
Imagine a one liter container into which 2.0 mol samples of gaseous substances A, B, and C are introduced. A and B react according to the following equation:
A(g) + B(g) ↔ 2C(g)
An increase in the temperature of the system would:
Drive the reaction to the right
Drive the reaction to the left
Have no effect on the reaction
The effect cannot be determined
For the reaction forming ammonia,
3H_{2}(g) + N_{2}(g) ↔ 2NH_{3}(g)
What effect will increasing the pressure by decreasing the volume of the system have on this system at equilibrium?
It will favor the formation of more ammonia
It will shift the equilibrium to the left
The [H_{2}] will increase
The [N_{2}] will increase
It will have no effect on the equilibrium concentrations
If the formation of ammonia, shown below, is exothermic at 25°C, what will be the effect of increasing the temperature of the system?
3H_{2}(g) + N_{2}(g) ↔ 2NH_{3}(g)
The equilibrium will shift to the right
The value of K will increase
The [H_{2}] will decrease
The value of K will decrease
Equilibrium is dependent on initial concentrations and equation stoichiometry, not on temperature. There will be no change.