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WorksheetsU7L1E2: Measuring Equilibrium
Total questions: 15
Worksheet time: 8mins
2 NO(g) + O2(g) ⇌ 2 NO2(g)
Fe3O4(s) + 4H2(g) <=> 3Fe(s) + 4H2O(g)
Kc =
What is the concentration equilibrium constant expression?
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
4Br2(g) + CH4(g) ↔ 4HBr(g) + CBr4(g)
What is the reaction/equation for this Kc expression
2N2 + O2 ⇌ 2NO
N2 + O2 ⇌ NO
NO ⇌ 2NO
N2 + O2 ⇌ 2NO
What is the equation/reaction for this Kc expression?
O3 ⇌ 3O2
2O3 ⇌ 3O2
2O3 ⇌ O2
3O2 ⇌ 2O3
If Kc is large that means the concentration of the __________ is high and therefore the concencentration of the __________ is low.
reactants, products
species, products
products, reactants
species, reactants
If Kc is small that means the concentration of the __________ is high and therefore the concencentration of the __________ is low.
reactants, products
species, products
products, reactants
species, reactants
The Kc expression for the reaction 2NH3 ⇌ N2 + 3H2
X(g) + Y(g) ⇄ XY(g)
In an experiment, X(g) and Y(g) were combined in a rigid container at constant temperature and allowed to react as shown in the equation above. The table provides the data collected during the experiment. Based on the data, which of the following claims is most likely correct?
The reaction was about to reach equilibrium 15 minutes after the reactants were combined because the concentrations of X and XY were almost the same.
The reaction reached equilibrium between 75 minutes and 155 minutes after the reactants were combined because the concentrations of X and XY remained constant.
The reaction did not reach equilibrium because only 86% of the initial concentration of X was consumed.
The reaction did not reach equilibrium because initially there was no XY inside the container.
X(g) + Y(g) ⇄ XY(g)
The particle diagram above illustrates the changes that take place when X(g) and Y(g) are placed inside a rigid container at constant temperature. Which of the following is a characteristic of a system at equilibrium that is best represented by the particle diagram?
The particle diagram shows that initially the reaction proceeds to the right to form products, which is a characteristic of a system at equilibrium.
The particle diagram shows that after 200s the rate of the reverse reaction is slower than the rate of the forward reaction, which is a characteristic of a system at equilibrium.
The particle diagram shows that after 200s there are no observable changes in the amounts of reactants and products, which is a characteristic of a system at equilibrium.
The particle diagram shows that between 0s and 200s the rates of the forward and reverse reactions are the same, which is a characteristic of a system at equilibrium.
