Chemical Reactions and Equilibria Quiz - Master Chemical Dynamics

Question 1 of 34

What is the general form of a chemical reaction?

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Reactants → Products

Products → Reactants

Reactants + Products

Reactants × Products

Question 2 of 34

Which law states that mass is neither created nor destroyed in a chemical reaction?

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Law of Conservation of Mass

Law of Definite Proportions

Law of Multiple Proportions

Law of Equilibrium

Question 3 of 34

What does the equilibrium constant (K) tell us about a reaction?

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The ratio of products to reactants at equilibrium

The rate of the reaction

The temperature of the reaction

The pressure of the reaction

Question 4 of 34

What effect does increasing the concentration of reactants have on the position of equilibrium?

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Shifts the equilibrium towards products

Shifts the equilibrium towards reactants

Has no effect

Shifts the equilibrium to the left

Question 5 of 34

According to Le Chatelier's principle, how does increasing pressure affect a reaction at equilibrium involving gases?

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Shifts the equilibrium towards the side with fewer gas molecules

Shifts the equilibrium towards the side with more gas molecules

Has no effect

Increases the rate of reaction

Question 6 of 34

What is a catalyst and how does it affect a chemical reaction?

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A substance that speeds up a reaction without being consumed

A substance that slows down a reaction

A substance that gets consumed in the reaction

A substance that changes the equilibrium position

Question 7 of 34

Which of the following is a characteristic of a dynamic equilibrium?

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The rate of the forward reaction equals the rate of the reverse reaction

The concentration of reactants decreases to zero

The concentrations of reactants and products are equal

The reaction has stopped completely

Question 8 of 34

What happens to the equilibrium constant (K) if the temperature of an exothermic reaction is increased?

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Decreases

Increases

Remains the same

Becomes zero

Question 9 of 34

In which type of reaction is energy typically released as heat?

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Exothermic reaction

Endothermic reaction

Reversible reaction

Irreversible reaction

Question 10 of 34

What does the term 'Le Chatelier's principle' describe?

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The response of a system at equilibrium to a disturbance

The rate of a chemical reaction

The energy changes in a reaction

The formation of products

Question 11 of 34

What happens to the equilibrium position when a catalyst is added to a reaction?

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No effect on the equilibrium position

Shifts the equilibrium towards the reactants

Shifts the equilibrium towards the products

Increases the concentration of reactants

Question 12 of 34

Which of the following is not a factor that affects equilibrium position?

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Concentration

Temperature

Pressure

Volume of the reaction mixture

Question 13 of 34

What is the expression for the equilibrium constant (Kc) for the reaction aA + bB ⇌ cC + dD?

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Kc = [C]^c [D]^d / [A]^a [B]^b

Kc = [A]^a [B]^b / [C]^c [D]^d

Kc = [A]^a [B]^b [C]^c [D]^d

Kc = [C]^c [D]^d [A]^a [B]^b

Question 14 of 34

What happens to the equilibrium constant if the reaction is reversed?

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The equilibrium constant becomes its reciprocal

The equilibrium constant doubles

The equilibrium constant halves

The equilibrium constant remains unchanged

Question 15 of 34

In which type of reaction does the equilibrium constant (Kc) depend on temperature?

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All reactions

Only exothermic reactions

Only endothermic reactions

Only reversible reactions

Question 16 of 34

What is the purpose of the reaction quotient (Q)?

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To predict the direction in which a reaction will proceed to reach equilibrium

To calculate the equilibrium constant

To measure the rate of the reaction

To determine the concentration of reactants

Question 17 of 34

Which of the following statements is true for a system at equilibrium?

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The concentrations of reactants and products remain constant

The rate of the forward reaction is zero

The rate of the reverse reaction is zero

The reaction has stopped completely

Question 18 of 34

What is the effect of adding an inert gas to a reaction at equilibrium?

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No effect on the position of equilibrium

Shifts the equilibrium towards the products

Shifts the equilibrium towards the reactants

Increases the rate of reaction

Question 19 of 34

What is the term for a reaction that proceeds in both forward and reverse directions?

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Reversible reaction

Irreversible reaction

Spontaneous reaction

Non-spontaneous reaction

Question 20 of 34

Which of the following conditions will not affect the equilibrium constant of a reaction?

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Temperature

Pressure

Concentration

Catalyst

Question 21 of 34

What is the significance of the equilibrium constant (K) being very large?

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The reaction favors the formation of products

The reaction favors the formation of reactants

The reaction is at a very slow rate

The reaction is irreversible

Question 22 of 34

In a dynamic equilibrium, how do the rates of the forward and reverse reactions compare?

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They are equal

The forward rate is faster

The reverse rate is faster

The rates are zero

Question 23 of 34

Which of the following changes will not affect the equilibrium position of a reaction?

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Change in temperature

Change in pressure

Change in concentration

Addition of a catalyst

Question 24 of 34

What is meant by the term 'chemical equilibrium'?

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The state where the rates of the forward and reverse reactions are equal

The state where all reactants have been converted to products

The state where no further reaction can occur

The state where products are formed only

Question 25 of 34

What is the effect of increasing temperature on the equilibrium of an endothermic reaction?

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Shifts the equilibrium towards the products

Shifts the equilibrium towards the reactants

No effect

Decreases the rate of reaction

Question 26 of 34

How does increasing the volume of the reaction container affect the equilibrium of a reaction involving gases?

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Shifts the equilibrium towards the side with more gas molecules

Shifts the equilibrium towards the side with fewer gas molecules

Has no effect

Increases the rate of reaction

Question 27 of 34

What is the effect of decreasing the concentration of a reactant on the equilibrium position?

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Shifts the equilibrium towards the reactants

Shifts the equilibrium towards the products

Has no effect

Increases the rate of reaction

Question 28 of 34

In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), how does increasing the pressure affect the equilibrium?

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Shifts the equilibrium towards the products

Shifts the equilibrium towards the reactants

Has no effect

Increases the concentration of hydrogen

Question 29 of 34

What is the reaction quotient (Q) for the reaction aA + bB ⇌ cC + dD if the reaction is not at equilibrium?

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Q = [C]^c [D]^d / [A]^a [B]^b

Q = [A]^a [B]^b / [C]^c [D]^d

Q = [A]^a [C]^c / [B]^b [D]^d

Q = [C]^c [A]^a / [D]^d [B]^b

Question 30 of 34

In a reaction at equilibrium, what does a reaction quotient (Q) value greater than the equilibrium constant (K) indicate?

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The reaction will shift towards the reactants

The reaction will shift towards the products

The reaction is at equilibrium

The equilibrium constant needs to be recalculated

Question 31 of 34

Which principle explains why a change in conditions causes a shift in the equilibrium position?

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Le Chatelier's principle

The Law of Conservation of Mass

Raoult's Law

Henry's Law

Question 32 of 34

What is the effect of adding more product to a system at equilibrium?

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Shifts the equilibrium towards the reactants

Shifts the equilibrium towards the products

No effect

Increases the rate of the reaction

Question 33 of 34

What type of reaction is represented by the equation CO2(g) + H2O(l) ⇌ H2CO3(aq)?

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Reversible reaction

Irreversible reaction

Exothermic reaction

Endothermic reaction

Question 34 of 34

Which of the following statements about equilibrium constants is false?

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The value of Kc is constant at a given temperature

Kc changes with changes in concentration

Kc is affected by changes in pressure

Kc is not affected by the presence of a catalyst

Chemical Reactions and Equilibria : Chemistry

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