Hydrogen gas and iodine gas are introduced into a flask, which is then sealed and allowed to reach dynamic chemical equilibrium.
The balanced equation is:
H2(g) + I2(g) ⇌ 2HI(g).
Which one of the graphs shows how the rates of the forward and reverse reactions change with time?
Which of the following is true regarding the concentration of products, for a chemical system at equilibrium?
The concentrations of products will not change because the limiting reagent is gone.
The concentrations of products will not change because the forward and reverse rates are equal.
The concentrations of products will not change because there are no more reactants.
The concentrations of products will change continually because of reversibility.
For the following system at equilibrium, which statement is INCORRECT?
Only one reaction will be affected by a change in temperature
The forward reaction is exothermic
The total change in enthalpy for the products is -184 kJ
It is a homogeneous equilibrium
Consider the amount (mol) vs. time graph for the closed system containing the gases of equation A at room temperature. The volume of the container is 1 dm3.
At which of the following time(s) is the the system NOT in equilibrium?
3 min
7 min
12 min
15 min
18 min
A disturbance to temperature was made at 10 minutes. Which reaction was favoured?
forward reaction
reverse reaction
Therefore, considering your answer above, what temperature change was made at 10 minutes?