WorksheetsCH 15-3: Le Chatelier's Principle
Total questions: 6
Worksheet time: 30mins
Hydrogen fluoride is produced by reacting hydrogen with fluorine.
H2(g) + F2(g) ⇌ 2HF(g) △H= -542.2 kJ
A stress that would shift the equilibrium towards the products would be to:
Add HF(g)
Remove H2(g)
Decrease the volume of the reaction vessel
Decrease the temperature of the reaction vessel
Identify the stress that was applied to the system at each of the given times ABCD (enter your answer as a 4 digit answer)
(a)
When PCl5(s) is heated, the given equilibrium is established.
PCl5(s) + 114.5 kJ ⇌ PCl3(l) + Cl2(g)
The mass of chlorine gas produced will be maximized when the temperature ___i___ and the volume of the flask ___ii___.
i) increases ii) increases
i) increases ii) decreases
i) decreases ii) increases
i) decreases ii) decreases
The formation of hydrogen iodide gas is represented by the given reaction:
H2(g) + I2(g) ⇌ 2HI(g)
Which of the following statements is true for the system above?
A decrease in pressure will not affect the reaction
An increase in pressure will favour the forward reaction
An increase in the concentration of H2 will not affect the reaction
An increase in the concentration of HI will favour the forward reaction
Some of the SO2(g) produced from the burning of coal and natural gas can react with NO2(g) in the atmosphere according to the equation:
SO2(g) + NO2(g) ⇌ NO(g) + SO3(g) △H= -41.9 kJ
The equilibrium concentration of SO3(g) in the reaction would be increased by
raising the temperature
adding a catalyst
removing SO2(g)
adding NO2(g)
For the equilibrium PCl5(g) ⇌ PCl3(g) + Cl2(g) the equilibrium constant at two temperatures is given below.
227°C Kc= 2.24
486°C Kc= 33.3
According to this information, as the temperature of the system increases, the equilibrium shifts
Left and the reaction is exothermic
Left and the reaction is endothermic
Right and the reaction is exothermic
Right and the reaction is endothermic
