The equilibrium constant is equal to 5.00 at 1300 K for the reaction: If initial concentrations are [SO2] = 0.60 M, [O2] = 0.20 M, and [SO3] = 0.50 M, the system is: A. at equilibrium B. Need to know the volume of the container before deciding. C. not at equilibrium and will shift to the right to achieve an equilibrium state D. not at equilibrium and will shift to the left to achieve an equilibrium state E. not at equilibrium and will remain in an unequilibrium state 2 SO2(g) + O2(g) ⇌ 2 SO3(g)
- The equilibrium constant is equal to 5.00 at 1300 K for the reaction: If initial concentrations are [SO2] = 0.60 M, [O2] = 0.20 M, and [SO3] = 0.50 M, the system is:
A. at equilibrium
B. Need to know the volume of the container before deciding.
C. not at equilibrium and will shift to the right to achieve an equilibrium state
D. not at equilibrium and will shift to the left to achieve an equilibrium state
E. not at equilibrium and will remain in an unequilibrium state
- 2 SO2(g) + O2(g) ⇌ 2 SO3(g)
Determine how the following changes affect the given equilblirium reaction that is held in a closed container.
A(g) + 2 B(s) ⇌ 3 C(g) + 3 D(s) ΔH°rxn = −0.25 kJ/mol
Adding some A(g)
Adding some D(s)
Removing some C(g)
Increasing the temperature
Halving the volume of the container
The following mechanism is proposed for the reaction
2 A2 + B2 → 2 C
A2 + B2 → R + C slow
A2 + R → C fast
What is the rate law for the overall reaction?
| A. |
rate = k[A2] |
|
| B. |
rate = k[A2]2 [B2] |
|
| C. |
rate = k[A2]2 |
|
| D. |
rate = k[R]2 |
|
| E. |
rate = k[A2][B2] |
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