The Haber process is a key step in the manufacture of fertilisers:
N2 (g) + 3H2 (g) 2NH3 (g) ΔH = -ve
Which is correct about the effect of increasing temperature for this reaction?
|
Effect on equilibrium position |
Effect on Kc |
A. |
Shifts left |
No change |
B. |
Shifts right |
No change |
C. |
Shifts right |
Increase |
D. |
Shifts left |
Decrease |
Which equation represents a reaction where the number of moles alone can not be used to calculate the value of Kc?
CH3CH2OH (aq) + CH3COOH (aq) CH3CH2OCOCH3 (aq) + H2O (l)
H2 (g) + I2 (g) 2HI (g)
2SO2 (g) + O2 (g) 2SO3 (g)
N2 (g) + O2 (g) 2NO (g)
When 0.20 mol NO, 0.08 mol H2 and 0.10 mol of H2O are placed in a 1.0 dm3 flask, the following equilibrium is established:
2NO (g) + 2H2 (g) N2 (g) + 2H2O (g)
At equilibrium, the concentration of H2 (g) was found to be 0.02 mol dm-3.
What is the correct calculation to work out Kc?
Nitrogen dioxide can form a dimer that can also break back down again as part of a reversible reaction:
N2O4 (g) NO2 (g) ΔH = +ve
The reaction reaches an equilibrium at temperature T, where Kc = 1
What is true for a higher temperature, T2?
|
Kc value |
ΔGθ value |
A. |
Increases |
Increases |
B. |
Decreases |
Increases |
C. |
Decreases |
Decreases |
D. |
Increases |
Decreases |
Which would be the correct way to plot a graph and then calculate ΔGθ from experimental data of Kc and temperature values?
ΔGθ = -RT ln K
|
y-axis |
x-axis |
ΔGθ = |
A. |
1 / T |
ln K |
-R x gradient |
B. |
ln K |
1 / T |
-R x gradient |
C. |
ln K |
1 / T |
R / gradient |
D. |
1 / T |
ln K |
R / gradient |