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- Multiple ChoicePlease save your changes before editing any questions.
Consider the following graph:
When equilibrium is reached, the rate of the forward reaction is
0.00 mol/min
0.25mol/min
1.0 mol/min
3.0 mol/min
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following equilibrium:
2NO2 (g) <-> N2O4 (g) + energy
The equilibrium will shift to the left as a result of
adding a catalyst.
increasing the volume.
removing some N2O4.
decreasing the temperature.
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following equilibrium:
N2 (g) + 3H2 (g) <-> 2NH3 (g) + energy
Certain conditions provide less than 10% yield of NH3 at equilibrium. Which of the following describes this equilibrium?
A
B
C
D
- Multiple ChoicePlease save your changes before editing any questions.
Which of the following best describes the relationship between Keq and temperature
for an endothermic reaction?
A
B
C
D
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following equilibrium:
2NO2(g) <-> N2O4(g)
A 1.00 L flask contains 0.030 mol NO2 and 0.040 mol N2O4 at equilibrium.
The value of Keq is
0.023
0.67
1.3
44
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following reaction:
2H2(g) + O2(g) <-> 2H2O(l)
What is the equilibrium constant expression for the reaction?
A
B
C
D
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following equilibrium:
2NOBr(g) <-> 2NO(g) + Br2(g) Keq = 6.4 X 10-2
At equilibrium, a 1.00 L flask contains 0.030 mol NOBr and 0.030 mol NO.
How many mol Br2 are present?
1.9 X 10-3 mol
6.4 X10-2 mol
3.0 X10-2 mol
4.7 X10-1 mol
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following equilibrium:
2NO(g) + O2(g) <-> 2NO2 (g) + energy
When the volume of the container is increased, the equilibrium shifts to the
left and Keq decreases.
right and Keq increases.
left and Keq remains constant.
right and Keq remains constant.
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following reaction:
2Hg(g) + O2(g) <-> 2HgO(s)
The equilibrium constant expression for the reaction is
A
B
C
D
- Multiple ChoicePlease save your changes before editing any questions.
The value of Keq changes when
a catalyst is added.
the temperature changes.
the surface area changes.
the concentration of reactants changes.
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following equilibrium:
PCl5(g) <-> PCl3(g) + Cl2(g)
A 1.00 L flask contains 0.0200 mol PCl5, 0.0500 mol PCl3 and 0.0500 mol Cl2 at
equilibrium. The value of Keq is
0.125
2.50
5.00
8.00
- Multiple ChoicePlease save your changes before editing any questions.
A
B
C
D
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following equilibrium:
2O3(g) <-> 3O2(g) Keq = 36
What is the concentration of O3 when the equilibrium concentration
Of O2 is 6.0 X 10-2 mol/L?
2.4 X 10-3 mol/L
4.0 X 10-2 mol/L
6.0 X 10-2 mo/L
9.0 X 10-2 mol/L
- Multiple ChoicePlease save your changes before editing any questions.
Which of the following does not apply to all chemical equilibrium systems?
They are closed.
The macroscopic properties are constant.
Forward and reverse reaction rates are equal.
There are equal concentrations of reactants and products.
- Multiple ChoicePlease save your changes before editing any questions.
Consider the following equilibrium:
H2 (g) + I2(g) <-> 2HI(g) Keq = 50.0
What is the value Keq for the reaction rewritten as:
2HI (g) <-> H2(g) + I2(g) Keq = ?
–50.0
0.0200
25.0
50.0