When gaseous dinitrogen pentoxide, N2O5 (g), decomposes at 358 K, the following equilibrium is established:
2N2O5 (g) ⇌ 4NO2 (g) + O2 (g)
2.0 mol of N2O5 (g) were placed in a 1.0 dm3 container and allowed to reach equilibrium. At equilibrium 1.0 mol of N2O5 (g) were present. What is the value of Kc?
0.125
1
2
8
Consider the following reversible reaction:
3O2 (g) ⇌ 2O3 (g)
What is the value of Kc when the equilibrium concentrations are [O2] = 4.0 mol dm-3 and [O3] = 4.0 mol dm-3 ?
0.25
4
16
64
Which if the following will shift the position of equilibrium to the right in the reaction shown?
2N2O5 (g) ⇌ 4NO2 (g) + O2 (g) ΔH = +219.2 kJ
I and II only
I and III only
II and III only
I, II and III
Hydrogen iodide decomposes to form hydrogen and iodine vapour.
2HI (g) ⇌ H2 (g) + I2 (g)
What is the effect of decreasing the volume of the equilibrium mixture at constant temperature?
The amount of H2 (g) remains the same but its concentration decreases
The forward reaction is favoured
The backward reaction is favoured
The value of Kc remains unchanged
A mixture of 0.40 mol of SO2 (g) and 0.40 mol of O2 (g) was placed in a 1 dm3 container. The following equilibrium took place:
2SO2 (g) + O2 (g) ⇌ 2SO3 (g)
At equilibrium the mixture contained 0.25 mol of O2 (g) .How many moles of SO2 (g) and SO3 (g) were present at equilibrium?
|
|
SO2 (g) / mol |
SO3 (g) / mol |
|
A |
0.25 |
0.15 |
|
B |
0.30 |
0.15 |
|
C |
0.10 |
0.30 |
|
D |
0.25 |
0.30 |
