WorksheetsRate of Reaction and Le Chatelier's Principle
Total questions: 22
Worksheet time: 44mins
Removing O2(g) will
Adding SO2(g) will
Adding SO3(g) will
Removing SO3(g) will
2SO2(g)+O2(g)⇌2SO3(g)
Increasing pressure of container will
shift equilibrium right
shift equilibrium left
slow rate of reaction
have no change
For N2 + 3H2 →2NH3 . When pressure is increased the equilibrium shift to right. Why?
To increase the amount of products
To reduce the pressure, as the right has less molecules
Kc will increase when it is shifted to the right
So it will increase the rate of reaction
N2O4 → NO2 (endothermic). Why when temperature is increased is the position of equilibrium shifted to the RIGHT?
Forward reaction is endothermic, thus reducing the temp
Forward reaction is exothermic, thus reducing the temp
Forward reaction is endothermic, thus increasing the temp
Forward reaction is exothermic, thus increasing the temp
SO2 + O2 <−> SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
heat + N2 + O2 ↔ 2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
N2 (g) + 3H2 (g) < -> 2NH3 (g) + Heat
add H2
Shift Left
Shift Right
N2 (g) + 3H2 (g) < -> 2NH3 (g) + Heat
Add Heat
Shift Left
Shift Right
Heat + N2O4 (g) ⇆ 2NO2 (g)
Add Heat
Shift Left
Shift Right
N2 (g) + 3H2 (g) < -> 2NH3 (g) + Heat
remove N2
Shift Left
Shift Right
