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Questions and Answers
What happens to the equilibrium position when temperature is increased in an exothermic reaction?
What happens to the equilibrium position when temperature is increased in an exothermic reaction?
In an industrial process, how does using a medium temperature affect reaction speed?
In an industrial process, how does using a medium temperature affect reaction speed?
What happens to the equilibrium position when a stress is applied to a system according to Le Châtelier’s Principle?
What happens to the equilibrium position when a stress is applied to a system according to Le Châtelier’s Principle?
According to Le Châtelier’s Principle, what occurs if more reactant is added to a system at equilibrium?
According to Le Châtelier’s Principle, what occurs if more reactant is added to a system at equilibrium?
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In the Haber process, what is the ratio of nitrogen to hydrogen gas used?
In the Haber process, what is the ratio of nitrogen to hydrogen gas used?
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How does a catalyst affect the position of equilibrium in a chemical reaction?
How does a catalyst affect the position of equilibrium in a chemical reaction?
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What will occur if the pressure of an equilibrium mixture is increased?
What will occur if the pressure of an equilibrium mixture is increased?
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What is the role of the iron catalyst in the Haber Process?
What is the role of the iron catalyst in the Haber Process?
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What can be observed about ammonia (NH3) in the equilibrium gas mixture during the Haber process?
What can be observed about ammonia (NH3) in the equilibrium gas mixture during the Haber process?
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What effect does reducing the temperature have on an endothermic reaction?
What effect does reducing the temperature have on an endothermic reaction?
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What happens when product is removed from an equilibrium mixture?
What happens when product is removed from an equilibrium mixture?
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What effect does adding nitrogen (N2) to the system have on the reaction quotient (Qc)?
What effect does adding nitrogen (N2) to the system have on the reaction quotient (Qc)?
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Why is it beneficial to continuously remove NH3 during the Haber process?
Why is it beneficial to continuously remove NH3 during the Haber process?
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In an exothermic system, how does a decrease in temperature affect product formation?
In an exothermic system, how does a decrease in temperature affect product formation?
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What is the equilibrium expression for the Haber process in terms of concentrations?
What is the equilibrium expression for the Haber process in terms of concentrations?
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Under the specified conditions of the Haber process, what range of temperature is typically used?
Under the specified conditions of the Haber process, what range of temperature is typically used?
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What effect does reducing the volume of a gas in a chemical reaction have on pressure and equilibrium position?
What effect does reducing the volume of a gas in a chemical reaction have on pressure and equilibrium position?
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In the Haber process, how does an increase in temperature affect the equilibrium position?
In the Haber process, how does an increase in temperature affect the equilibrium position?
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Which statement is true regarding the equilibrium constant of a reaction?
Which statement is true regarding the equilibrium constant of a reaction?
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What is the impact of using a catalyst in a chemical reaction regarding equilibrium?
What is the impact of using a catalyst in a chemical reaction regarding equilibrium?
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For the reaction H2(g) + I2(g) ⇌ 2 HI(g), how does changing the pressure affect the equilibrium?
For the reaction H2(g) + I2(g) ⇌ 2 HI(g), how does changing the pressure affect the equilibrium?
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In an endothermic reaction, increasing the temperature has what effect on the equilibrium position?
In an endothermic reaction, increasing the temperature has what effect on the equilibrium position?
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In the reaction C(s) + H2O(g) ⇌ CO(g) + H2(g), how does increasing the pressure impact the equilibrium?
In the reaction C(s) + H2O(g) ⇌ CO(g) + H2(g), how does increasing the pressure impact the equilibrium?
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What does Le Chatelier’s Principle state regarding changes in reaction conditions?
What does Le Chatelier’s Principle state regarding changes in reaction conditions?
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What is the value of $[NO]$ when the equilibrium concentrations are $[NO2] = 5.0 \times 10^{-2} M$ and $[O2] = 1.0 \times 10^{-3} M$?
What is the value of $[NO]$ when the equilibrium concentrations are $[NO2] = 5.0 \times 10^{-2} M$ and $[O2] = 1.0 \times 10^{-3} M$?
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What happens to the equilibrium constant $K_c$ when the concentration of reactants is reduced?
What happens to the equilibrium constant $K_c$ when the concentration of reactants is reduced?
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At equilibrium, if $[H2]$ and $[I2]$ both are calculated to be $0.021 M$, what is the concentration of $[HI]$?
At equilibrium, if $[H2]$ and $[I2]$ both are calculated to be $0.021 M$, what is the concentration of $[HI]$?
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When expanding the equilibrium expression into a quadratic equation, which terms correspond to coefficients a, b, and c?
When expanding the equilibrium expression into a quadratic equation, which terms correspond to coefficients a, b, and c?
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In the reaction $H2(g) + I2(g) \rightarrow 2 HI(g)$, if $K_c = 57.0$ at 700 K, what is the main consideration before using the quadratic formula?
In the reaction $H2(g) + I2(g) \rightarrow 2 HI(g)$, if $K_c = 57.0$ at 700 K, what is the main consideration before using the quadratic formula?
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For the equilibrium expression $K_c = \frac{[HI]^2}{[H2][I2]}$, if $K_c$ is known to be 57.0, what does this imply about the favorability of the formation of products?
For the equilibrium expression $K_c = \frac{[HI]^2}{[H2][I2]}$, if $K_c$ is known to be 57.0, what does this imply about the favorability of the formation of products?
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If the forward reaction is represented as $2 NO(g) + O2(g) \rightarrow 2 NO2(g)$, how would an increase in temperature affect $K_c$, assuming the reaction is exothermic?
If the forward reaction is represented as $2 NO(g) + O2(g) \rightarrow 2 NO2(g)$, how would an increase in temperature affect $K_c$, assuming the reaction is exothermic?
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In the equilibrium expression $K_c = \frac{[NO2]^2}{[NO]^2 [O2]}$, what should be the initial concentrations of $NO$ and $O2$ to achieve equilibrium concentrations of $[NO2] = 0.05 M$ and $K_c = 6.9 \times 10^5$?
In the equilibrium expression $K_c = \frac{[NO2]^2}{[NO]^2 [O2]}$, what should be the initial concentrations of $NO$ and $O2$ to achieve equilibrium concentrations of $[NO2] = 0.05 M$ and $K_c = 6.9 \times 10^5$?
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Description
Test your understanding of chemical equilibrium with this quiz on MED-102. You will perform calculations, predict disturbances, and discuss the relationship between kinetics and equilibrium. Challenge yourself with example reactions and see if you can simplify complex equations.
