Test Your Chemistry Knowledge Now

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Test Your Chemistry Knowledge Now - Quiz

How strong are your fundamentals of Chemistry? Can you prove your knowledge? How about you take an online test and show us how much you know. So, let's get started.


Questions and Answers
  • 1. 

    Select the factors that affect the reaction rate:

    • A.

      Physical state reactants 

    • B.

      Presence of a catalyst 

    • C.

      Reactant concentration 

    • D.

      All of the above 

    Correct Answer
    D. All of the above 
    Explanation
    The factors that affect the reaction rate include the physical state of the reactants, the presence of a catalyst, and the reactant concentration. The physical state of the reactants can affect the surface area available for the reaction to occur, with greater surface area leading to a faster reaction rate. Catalysts can increase the rate of reaction by providing an alternative pathway with lower activation energy. The reactant concentration affects the frequency of collisions between reactant particles, with higher concentration leading to more collisions and a faster reaction rate. Therefore, all of these factors play a role in determining the reaction rate.

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  • 2. 

    The rate of the appearance of NO2=6 molar/sec what is the rate of appearance of O2?

    • A.

      1/2

    • B.

      -1/2

    • C.

      24

    • D.

      -24

    Correct Answer
    A. 1/2
    Explanation
    The rate of appearance of NO2 is given as 6 molar/sec. Since the balanced chemical equation for the reaction is not provided, we cannot determine the stoichiometry of the reaction. Therefore, we cannot directly calculate the rate of appearance of O2. Without further information, it is not possible to determine the rate of appearance of O2.

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  • 3. 

    Rate of appearance of NO2=6molar/sec, what is the rate of disappearance of N2O5

    • A.

      -3

    • B.

      3

    • C.

      12

    • D.

      -12

    Correct Answer
    B. 3
    Explanation
    The rate of appearance of NO2 is given as 6 molar/sec. Since the reaction involves the disappearance of N2O5, the rate of disappearance of N2O5 can be assumed to be equal to the rate of appearance of NO2. Therefore, the rate of disappearance of N2O5 is also 6 molar/sec.

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  • 4. 

    If you have the equation below determine the relationship between the disappearance ofN2O5 and the appearance of O2

    • A.

      -1/2(N2O5/t)=O2/t

    • B.

      1/2(N2O5/t)=-O2/t

    • C.

      (N2O5/t)=-1/2(O2/t)

    • D.

      (N2O5/t)=O2/t

    Correct Answer
    A. -1/2(N2O5/t)=O2/t
    Explanation
    The given equation shows that the disappearance of N2O5 is directly proportional to the appearance of O2. This means that as the amount of N2O5 decreases over time, the amount of O2 increases at the same rate. The negative sign in front of the 1/2 indicates that the two quantities have an inverse relationship, meaning that as one increases, the other decreases. Therefore, the correct answer is -1/2(N2O5/t) = O2/t.

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  • 5. 

    Rate=k[A]^x[B]^y If X=1 and Y=2 what is the overall order of the reaction?

    • A.

      2

    • B.

      3

    • C.

      1

    • D.

      Non of the above 

    Correct Answer
    B. 3
    Explanation
    The overall order of a reaction is determined by the sum of the exponents (x and y) in the rate equation. In this case, since X=1 and Y=2, the sum of the exponents is 1+2=3. Therefore, the overall order of the reaction is 3.

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  • 6. 

    If you have the following data: identify the order of y?

    • A.

      2

    • B.

      1

    • C.

      3

    • D.

      Non of the above 

    Correct Answer
    B. 1
    Explanation
    The correct answer is 1 because it is the second number in the given data set.

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  • 7. 

    If k[3A]^x and the rate law is 27k[A]^x what is the order of x?

    • A.

      1

    • B.

      3

    • C.

      2

    • D.

      0

    Correct Answer
    B. 3
    Explanation
    The rate law is given as 27k[A]^x, which means the rate of the reaction is directly proportional to the concentration of A raised to the power of x. Since k is raised to the power of 3A, it can be inferred that x must be equal to 3 in order for the rate law to be consistent. Therefore, the order of x is 3.

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  • 8. 

    Calculate the rate constant of this reaction:

    • A.

      1.2*10^4 M^-1.s^-2

    • B.

      1.2*10^4 M^-2.s^-1

    • C.

      2.4*10^4 M^-1.s^-2

    • D.

      2.4*10^4 M^-2.s^-1

    Correct Answer
    B. 1.2*10^4 M^-2.s^-1
    Explanation
    The rate constant of a reaction represents the speed at which the reaction occurs. It is a constant that relates the concentrations of the reactants to the rate of the reaction. In this case, the correct answer is 1.2*10^4 M^-2.s^-1. This means that the rate of the reaction is proportional to the square of the concentration of the reactants. The units M^-2.s^-1 indicate that the concentration is in moles per liter and the time is in seconds.

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  • 9. 

    What is the rate of the reaction when [No]=0.15M and [Br2]= 0.25M  hints: you need to find x and y first. k=1.2*10^4 M^-2.s^-1

    • A.

      67.5M.s^-1

    • B.

      67.5M.s

    • C.

      64.5M.s^-1

    • D.

      64.5M^-1.s

    Correct Answer
    A. 67.5M.s^-1
  • 10. 

    Which of the following equations is a first order equation?

    • A.

      1/[A]t=kt+1/[A]0

    • B.

      [A]t=-kt+[A]0

    • C.

      [A]t=kt-[A]0

    • D.

      Ln[A]t=-kt+ln[A]0

    Correct Answer
    D. Ln[A]t=-kt+ln[A]0
    Explanation
    The equation ln[A]t=-kt+ln[A]0 is a first order equation because it is a linear equation in the form y=mx+c, where y is ln[A]t, x is t, m is -k, and c is ln[A]0. First order equations have a linear relationship between the dependent variable (ln[A]t) and the independent variable (t), with a constant rate of change (-k).

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  • 11. 

    The reaction 2A=B has a rate constant of 2.8*10^-2 s^-1 at 80c, How long will it take for A to decrease from 0.88M to 0.14M. Fine the order of A

    • A.

      66s , 1st order 

    • B.

      66s ,0th order 

    • C.

      65.8s , 2nd order 

    • D.

      100s, 1st order 

    Correct Answer
    A. 66s , 1st order 
    Explanation
    The given question asks to find the order of A in the reaction 2A=B. The rate constant of the reaction is given as 2.8*10^-2 s^-1 at 80°C. To find the order of A, we need to determine the relationship between the rate of the reaction and the concentration of A. Since the reaction is first order with respect to A, it means that the rate of the reaction is directly proportional to the concentration of A. Therefore, as A decreases from 0.88M to 0.14M, it will take 66 seconds for the concentration to decrease. Hence, the answer is "66s, 1st order".

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  • 12. 

    The higher the activation energy is the slower the reaction gets.

    • A.

      True

    • B.

      False

    Correct Answer
    A. True
    Explanation
    The statement is true because activation energy is the minimum amount of energy required for a chemical reaction to occur. If the activation energy is high, it means that more energy is needed for the reactants to overcome the energy barrier and form products. This results in a slower reaction rate as fewer reactant molecules possess the required energy. Conversely, if the activation energy is low, more reactant molecules have enough energy to react, leading to a faster reaction rate. Therefore, the higher the activation energy, the slower the reaction gets.

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  • 13. 

    What is the relationship between the rate and each of the following depending on Arrhenius equation: 1)T 2)A 3)Ea

    • A.

      1)increases  2)increases  3)decrease 

    • B.

      1)increases  2)decrease   3)decrease 

    • C.

      1)increases  2)increases  3)increase 

    • D.

      1)decreases   2)increases  3)decrease 

    Correct Answer
    A. 1)increases  2)increases  3)decrease 
    Explanation
    According to the Arrhenius equation, the rate of a reaction is directly proportional to the temperature (T) and the value of the pre-exponential factor (A), and inversely proportional to the activation energy (Ea). Therefore, as the temperature increases, the rate of the reaction also increases. Similarly, as the value of the pre-exponential factor increases, the rate of the reaction increases. On the other hand, as the activation energy decreases, the rate of the reaction decreases.

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  • Current Version
  • Mar 21, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • Mar 08, 2021
    Quiz Created by
    Themes
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