Can you pass this Chemical Kinetics Test? Trivia Quiz

1. A reaction involving two different reactants can never be:

Unimolecular Reaction

First order reaction

Second order reaction

Bimolecular reaction

A unimolecular reaction involves the decomposition or rearrangement of a single molecule. It does not involve the interaction between two different reactants. Therefore, a reaction involving two different reactants can never be a unimolecular reaction.

Explanation

A unimolecular reaction involves the decomposition or rearrangement of a single molecule. It does not involve the interaction between two different reactants. Therefore, a reaction involving two different reactants can never be a unimolecular reaction.

2. A reaction was found to be second order with respect to concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will:

Become three times

Increase by factor of 4

Become two times

Remains Unchanged

In a second-order reaction, the rate of the reaction is directly proportional to the square of the concentration of the reactant. Therefore, if the concentration of carbon monoxide is doubled, the rate of the reaction will increase by a factor of 2^2, which is 4. This means that the rate of the reaction will increase by a factor of 4.

Explanation

In a second-order reaction, the rate of the reaction is directly proportional to the square of the concentration of the reactant. Therefore, if the concentration of carbon monoxide is doubled, the rate of the reaction will increase by a factor of 2^2, which is 4. This means that the rate of the reaction will increase by a factor of 4.

3. The conversion of molecules X and Y follows second order kinetics. If concentration of X is increased to three times, how will it affect the rate of formation of Y?

Decrease the rate of time for the conversion of X to Y.

Increase the rate of time for the conversion of X to Y.

No change in rate of time for the conversion of X to Y.

No dependency on time.

When the concentration of X is increased to three times, it will lead to an increase in the rate of formation of Y. This is because the conversion of X and Y follows second order kinetics, which means that the rate of the reaction is directly proportional to the square of the concentration of X. Therefore, when the concentration of X is increased, the rate of formation of Y will also increase.

Explanation

When the concentration of X is increased to three times, it will lead to an increase in the rate of formation of Y. This is because the conversion of X and Y follows second order kinetics, which means that the rate of the reaction is directly proportional to the square of the concentration of X. Therefore, when the concentration of X is increased, the rate of formation of Y will also increase.

4. Predict the order of reaction, looking onto the figure:

Zero

One

Two

Three

The graph illustrates a linear relationship between the rate of reaction and the concentration of the reactant, indicating that the rate increases directly in proportion to the concentration. This pattern is characteristic of a first-order reaction, where the reaction rate is directly proportional to the concentration of one reactant. Therefore, the order of the reaction depicted in the graph is first-order.

Explanation

The graph illustrates a linear relationship between the rate of reaction and the concentration of the reactant, indicating that the rate increases directly in proportion to the concentration. This pattern is characteristic of a first-order reaction, where the reaction rate is directly proportional to the concentration of one reactant. Therefore, the order of the reaction depicted in the graph is first-order.

5. In a reaction, A + B Product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled, rate law for the reaction can be written as:

Rate = k [A] [B]

Rate = k [A]2 [B]

Rate = k [A] [B]2

Rate = k [A]2 [B]2

The given information states that when the concentration of B is doubled, the rate is also doubled. This suggests that the rate is directly proportional to the concentration of B. Additionally, when the concentrations of both reactants A and B are doubled, the rate increases by a factor of 8. This indicates that the rate is directly proportional to the concentration of both A and B. Therefore, the rate law for the reaction can be written as Rate = k [A]2 [B], where k is the rate constant.

Explanation

The given information states that when the concentration of B is doubled, the rate is also doubled. This suggests that the rate is directly proportional to the concentration of B. Additionally, when the concentrations of both reactants A and B are doubled, the rate increases by a factor of 8. This indicates that the rate is directly proportional to the concentration of both A and B. Therefore, the rate law for the reaction can be written as Rate = k [A]2 [B], where k is the rate constant.

6. The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of reaction with respect to reactant B is:

-1

1

-2

2

The rate of reaction between reactants A and B is said to decrease by a factor of 4 when the concentration of reactant B is doubled. This suggests that the rate of reaction is inversely proportional to the concentration of reactant B. In other words, as the concentration of B increases, the rate of reaction decreases. This indicates that the reaction is second order with respect to reactant B. Therefore, the answer is -2.

Explanation

The rate of reaction between reactants A and B is said to decrease by a factor of 4 when the concentration of reactant B is doubled. This suggests that the rate of reaction is inversely proportional to the concentration of reactant B. In other words, as the concentration of B increases, the rate of reaction decreases. This indicates that the reaction is second order with respect to reactant B. Therefore, the answer is -2.

7. If a reaction is 50% complete in 2 hours and 75% complete in 4 hours. What is the order of the reaction:

First order reaction

Third order reaction

Zero order reaction

Second order reaction

The given information states that the reaction is 50% complete in 2 hours and 75% complete in 4 hours. In a first-order reaction, the rate of reaction is directly proportional to the concentration of the reactant. As the reaction progresses, the concentration of the reactant decreases exponentially. The fact that the reaction is 50% complete in 2 hours and 75% complete in 4 hours suggests that the reaction is proceeding at a constant rate, indicating a first-order reaction.

Explanation

The given information states that the reaction is 50% complete in 2 hours and 75% complete in 4 hours. In a first-order reaction, the rate of reaction is directly proportional to the concentration of the reactant. As the reaction progresses, the concentration of the reactant decreases exponentially. The fact that the reaction is 50% complete in 2 hours and 75% complete in 4 hours suggests that the reaction is proceeding at a constant rate, indicating a first-order reaction.

8. Consider a reaction, aG + bH Products. When concentration of both the reactants G and H is doubled, the rate increases by eight times. However, when the concentration of G is doubled keeping the concentration of H fixed, the rate is doubled. The overall order of the reaction is:

0

1

2

3

In this reaction, when the concentration of both reactants G and H is doubled, the rate increases by eight times. This suggests that the rate is directly proportional to the square of the concentration of both reactants. Furthermore, when the concentration of G is doubled while keeping the concentration of H fixed, the rate is doubled. This indicates that the rate is directly proportional to the concentration of G. Therefore, the overall order of the reaction is 3, which means that the rate is proportional to the cube of the concentration of G and H.

Explanation

In this reaction, when the concentration of both reactants G and H is doubled, the rate increases by eight times. This suggests that the rate is directly proportional to the square of the concentration of both reactants. Furthermore, when the concentration of G is doubled while keeping the concentration of H fixed, the rate is doubled. This indicates that the rate is directly proportional to the concentration of G. Therefore, the overall order of the reaction is 3, which means that the rate is proportional to the cube of the concentration of G and H.

9. The rate of a chemical reaction doubles for every 10°C rise of temperature. If the temperature is raised by 50°C, the rate of the reaction increases by about:

10 times

24 times

32 times

64 times

The rate of a chemical reaction is known to double for every 10°C rise in temperature. Therefore, for a 50°C rise in temperature, the rate of the reaction would double 5 times (50°C/10°C = 5). Since the rate doubles each time, the rate of the reaction would increase by 2^5 = 32 times.

Explanation

The rate of a chemical reaction is known to double for every 10°C rise in temperature. Therefore, for a 50°C rise in temperature, the rate of the reaction would double 5 times (50°C/10°C = 5). Since the rate doubles each time, the rate of the reaction would increase by 2^5 = 32 times.

10. When a bio chemical reaction is carried out in laboratory; outside the human body in the absence of enzyme, then the rate of reaction obtained is 10^–6 times, than activation energy of reaction in the presence of enzyme is:

6/RT

P is required

Different from Ea obtained in laboratory

Can’t say anything

When a biochemical reaction is carried out in the laboratory without the presence of an enzyme, the rate of reaction obtained is different from the activation energy (Ea) obtained in the laboratory. This suggests that the presence of an enzyme significantly affects the rate of reaction. Enzymes lower the activation energy barrier, allowing the reaction to occur at a faster rate. Therefore, the activation energy in the presence of an enzyme is different from the activation energy obtained in the laboratory without the enzyme.

Explanation

When a biochemical reaction is carried out in the laboratory without the presence of an enzyme, the rate of reaction obtained is different from the activation energy (Ea) obtained in the laboratory. This suggests that the presence of an enzyme significantly affects the rate of reaction. Enzymes lower the activation energy barrier, allowing the reaction to occur at a faster rate. Therefore, the activation energy in the presence of an enzyme is different from the activation energy obtained in the laboratory without the enzyme.

11. In the reaction: BrO₃^– (aq) + 5Br^– (aq) + 6H⁺ 3Br₂ (l) + 3H₂O(l) The rate of appearance of bromine (Br₂) is related to the rate of disappearance of bromide ions as

The rate of appearance of bromine (Br2) is related to the rate of disappearance of bromide ions because bromide ions (Br-) are being oxidized to form bromine (Br2) in the reaction. As the reaction progresses, the concentration of bromide ions decreases, resulting in a decrease in the rate of disappearance of bromide ions. At the same time, the concentration of bromine increases, leading to an increase in the rate of appearance of bromine. Therefore, the rate of appearance of bromine is directly proportional to the rate of disappearance of bromide ions in this reaction.

Explanation

The rate of appearance of bromine (Br2) is related to the rate of disappearance of bromide ions because bromide ions (Br-) are being oxidized to form bromine (Br2) in the reaction. As the reaction progresses, the concentration of bromide ions decreases, resulting in a decrease in the rate of disappearance of bromide ions. At the same time, the concentration of bromine increases, leading to an increase in the rate of appearance of bromine. Therefore, the rate of appearance of bromine is directly proportional to the rate of disappearance of bromide ions in this reaction.

12. For the reaction N₂O₅(g) 2NO₂(g) + 1/2O₂(g) the value of rate of disappearance of N₂O₅ is given as 6.25 m 10^–3 mol L^–1 s^–1. The rate of formation of NO₂ and O₂ is given respectively as:

1.25 x 10-2 mol L-1 s-1 and 3.125 x 10-3 mol L-1 s-1

1.25 x 10-3 mol L-1 s-1 and 3.125 x 10-3 mol L-1 s-1

6.25 x 10-2 mol L-1 s-1 and 3.125 x 10-3 mol L-1 s-1

6.25 x 10-3 mol L-1 s-1 and 3.125 x 10-3 mol L-1 s-1

The rate of formation of NO2 and O2 can be determined by using the stoichiometry of the reaction. From the balanced equation, we can see that for every 1 mole of N2O5 that disappears, 2 moles of NO2 and 1/2 mole of O2 are formed. Therefore, the rate of formation of NO2 is half the rate of disappearance of N2O5, which is 1.25 x 10-2 mol L-1 s-1. Similarly, the rate of formation of O2 is also half the rate of disappearance of N2O5, which is 3.125 x 10-3 mol L-1 s-1.

Explanation

The rate of formation of NO2 and O2 can be determined by using the stoichiometry of the reaction. From the balanced equation, we can see that for every 1 mole of N2O5 that disappears, 2 moles of NO2 and 1/2 mole of O2 are formed. Therefore, the rate of formation of NO2 is half the rate of disappearance of N2O5, which is 1.25 x 10-2 mol L-1 s-1. Similarly, the rate of formation of O2 is also half the rate of disappearance of N2O5, which is 3.125 x 10-3 mol L-1 s-1.

13. Which of the following statement for order of reaction is not correct?

Order can be determined experimentally.

Order of a reaction is equal to the sum of the power of concentration terms in differential rate law.

It is not affected with the stoichiometric coefficients of the reactants.

Order can be fractional.

Order of a reaction is equal to the sum of the power of concentration terms in differential rate law.

This statement can be misleading because it suggests that the order is directly related to the stoichiometric coefficients, which is not necessarily true. The order of a reaction must be determined experimentally and is not always equal to the sum of the stoichiometric coefficients in the balanced chemical equation.

Explanation

Order of a reaction is equal to the sum of the power of concentration terms in differential rate law.

This statement can be misleading because it suggests that the order is directly related to the stoichiometric coefficients, which is not necessarily true. The order of a reaction must be determined experimentally and is not always equal to the sum of the stoichiometric coefficients in the balanced chemical equation.

14. A follows first-order reaction, (A) product

Concentration of A, changes from 0.1 M to 0.025 M in 40 minutes. Find the rate of reaction of A when the concentration of A is 0.01 M.

1.73 x 10-4 M min-1

1.73 x 10-5 M min-1

3.47 x 10-5 M min-1

3.47 x 10-4 M min-1

The rate of reaction can be determined using the first-order reaction rate equation, which is rate = k[A]. Given that the concentration of A changes from 0.1 M to 0.025 M in 40 minutes, we can use this information to calculate the rate constant (k) using the integrated rate law for a first-order reaction. Once we have the rate constant, we can plug in the concentration of A (0.01 M) into the rate equation to find the rate of reaction. The correct answer, 3.47 x 10^-4 M min-1, is obtained by performing these calculations.

Explanation

The rate of reaction can be determined using the first-order reaction rate equation, which is rate = k[A]. Given that the concentration of A changes from 0.1 M to 0.025 M in 40 minutes, we can use this information to calculate the rate constant (k) using the integrated rate law for a first-order reaction. Once we have the rate constant, we can plug in the concentration of A (0.01 M) into the rate equation to find the rate of reaction. The correct answer, 3.47 x 10^-4 M min-1, is obtained by performing these calculations.

15. For the reaction: 2A + B 3C + D Which of the following does not express the reaction rate?

The reaction rate is the speed at which reactants are consumed or products are formed. In this case, the options provided are expressions for the reaction rate. Therefore, it is not possible to determine which of the options does not express the reaction rate without knowing the options themselves.

Explanation

The reaction rate is the speed at which reactants are consumed or products are formed. In this case, the options provided are expressions for the reaction rate. Therefore, it is not possible to determine which of the options does not express the reaction rate without knowing the options themselves.

Can You Pass This Chemical Kinetics Test? Trivia Quiz