Which of the following statements are incorrect?
1) Gases are not included in the equilibrium constant expression.
2) Equilibrium constant can be increased by adding a catalyst
3) Large equilibrium constant favors reactants
4) Equilibrium is typically achieved in a very short time
5) Equilibrium can only be achieved if reactants are mixed in stoichiometric proportions
I think that it's only statement 4.. i was thinking about 3 too but I left it to stay on the safeside. I'd love to get someone elses point of view on this problem
1) Gases are not included in the equilibrium constant expression.They are included so this is incorrect.
2) Equilibrium constant can be increased by adding a catalyst.They can not be changed by adding a catalyst so this is incorrect
3) Large equilibrium constant favors reactantsLarge Keq favors products so this is incorrect.
4) Equilibrium is typically achieved in a very short time Equilibrium time varies; therefore, this is incorrect.
5) Equilibrium can only be achieved if reactants are mixed in stoichiometric proportions This is incorrect.
oh wow........ :[ thanks Dr. Bob
To determine which statements are correct or incorrect, let's go through each statement and explain them one by one:
1) Gases are not included in the equilibrium constant expression.
This statement is incorrect. Gases are indeed included in the equilibrium constant expression. The equilibrium constant expression, denoted as Kc, relates the concentrations (or partial pressures) of reactants and products at equilibrium. Every species in the balanced chemical equation, including gases, is included in the equilibrium constant expression.
2) Equilibrium constant can be increased by adding a catalyst.
This statement is incorrect. Adding a catalyst does not affect the value of the equilibrium constant. A catalyst is a substance that speeds up the rate of a chemical reaction but does not participate in the reaction or alter the position of equilibrium. Thus, the equilibrium constant remains the same in the presence of a catalyst.
3) Large equilibrium constant favors reactants.
This statement is incorrect. The equilibrium constant (Kc) represents the ratio of the concentrations (or partial pressures) of products to reactants at equilibrium. A large equilibrium constant indicates that the amount of products is favored at equilibrium, meaning the reaction has shifted to the right. On the other hand, a small equilibrium constant indicates that the amount of reactants is favored at equilibrium, and the reaction has shifted to the left.
4) Equilibrium is typically achieved in a very short time.
This statement is incorrect. The time required to reach equilibrium varies depending on factors such as the nature of the reactants, concentration, temperature, and presence of catalysts. Some reactions may reach equilibrium quickly, while others may take hours, days, or even longer to reach equilibrium.
5) Equilibrium can only be achieved if reactants are mixed in stoichiometric proportions.
This statement is incorrect. Equilibrium can be achieved regardless of whether the reactants are mixed in stoichiometric proportions. Stoichiometric proportions refer to the exact molar ratio of reactants as dictated by the balanced chemical equation. While the equilibrium composition may vary based on the initial concentrations of reactants, equilibrium can still be reached even if the reactants are not initially mixed in stoichiometric proportions.
Therefore, statements 1, 2, 3, and 5 are incorrect. Statement 4 (Equilibrium is typically achieved in a very short time) is also incorrect.