Chemistry- Chemical Reactions And Collision Theory Test

33 Questions | Total Attempts: 150

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Chemistry- Chemical Reactions And Collision Theory Test

If you are a chemistry student, this test is perfect for testing your subject knowledge. It has questions about various chemical reactions, the role of enzymes, collision theory, etc. Let's see if you can score a 100% or not. All the best!


Questions and Answers
  • 1. 
    Consider the following reversible, exothermic chemical reaction: 2C2H2(g) + 5O2(g) ↔4CO2(g) + 2H2O(g) All BUT one of the conditions will cause equilibrium to shift right and produce more of the products. Which change will cause the reaction to shift to the left?
    • A. 

      Adding oxygen

    • B. 

      Adding CO2

    • C. 

      Increasing the pressure

    • D. 

      Decreasing the temperature

  • 2. 
    Which one do you like? Collision theory states that when two molecules collide with each other with sufficient energy and hit in the proper orientation, a bond is formed. Which action will increase the rate of reaction in a closed container?
    • A. 

      Adding an inert gas

    • B. 

      Expand the volume

    • C. 

      Increase the temperature

    • D. 

      Decrease the concentration

  • 3. 
    When a mixture is stirred
    • A. 

      The rate of dissolving stops

    • B. 

      The rate of dissolving will increase

    • C. 

      The rate of dissolving will decrease

    • D. 

      The rate of dissolving will remain constant

  • 4. 
    All BUT one action would increase the rate at which solid metal will react with a acid solution. That is
    • A. 

      Decrease the molarity of the acid

    • B. 

      Break the metal into smaller pieces

    • C. 

      Increase the temperature of the solution

    • D. 

      Increase the concentration of the acid solution

  • 5. 
    Kc =[CO2]2/[CO]2[O2] is the equilibrium constant for which chemical reaction?
    • A. 

      CO + O2 ↔ CO2

    • B. 

      2CO + O2 ↔ 2CO2

    • C. 

      2CO2 ↔ 2CO + O2

    • D. 

      CO + 1/2 O2 ↔ CO2

  • 6. 
    In cells, __________ are proteins that are needed to lower the amount of energy required to start chemical reactions.
    • A. 

      Acid

    • B. 

      Enzymes

    • C. 

      Products

    • D. 

      Substrates

  • 7. 
    Jake wants to quickly dissolve Gatorade in a pitcher. What would help Jake INCREASE the rate at which his Gatorade dissolves?
    • A. 

      Adding sugar

    • B. 

      Cooling the mixture

    • C. 

      Adding more Gatorade

    • D. 

      Stirring the mixture

  • 8. 
    CO (g) + 2H2 (g) ↔ CH3OH (g) The equilibrium reaction can be shifted to form more products by _____________.
    • A. 

      Decreasing the pressure.

    • B. 

      Adding more hydrogen.

    • C. 

      Adding more methanol (CH3OH (g)).

    • D. 

      Adding a catalyst.

  • 9. 
    Hydrogen peroxide is a harmful by-product of normal metabolic activity. In order to prevent damage, hydrogen peroxide must be broken down into water and oxygen quickly. What would speed up the decomposition of hydrogen peroxide?
    • A. 

      A catalyst

    • B. 

      bubbling in oxygen

    • C. 

      Decreasing the temperature

    • D. 

      Adding more hydrogen peroxide

  • 10. 
    Why do we say that "an enzyme is reusable"?
    • A. 

      The enzyme does not actively take part in the reaction. It just indicates that the reaction is complete.

    • B. 

      Enzymes react with the substrate to form products and become denatured in the process.

    • C. 

      Enzymes ensure that the reaction continues without inhibition even if conditions such as temperature and PH are changed.

    • D. 

      The products of the reaction are released from the active sites of the enzyme, allowing other substrate molecules to bind with the sites.

  • 11. 
    Collision theory states that for a chemical reaction to occur the reacting particles must collide with one another. In order for collisions to be successful, reacting particles must collide with sufficient energy and in the correct orientation to produce a temporary intermediate product, the activated complex. ____________ energy is the minimum energy required for a successful collision.
    • A. 

      Activation

    • B. 

      Collision

    • C. 

      Kinetic

    • D. 

      Potential

  • 12. 
    Increasing the temperature, as noted in the graph, increases the rate of this chemical reaction. What is the relationship between increased temperature and activation energy in a typical chemical reaction?
    • A. 

      As the kinetic energy of the substances increases, the overall activation energy also increases.

    • B. 

      The proportion of collisions that can overcome the activation energy for the reaction increases with temperature.

    • C. 

      Although the average kinetic energy of the colliding substances increases, this has no influence on activation energy.

    • D. 

      The proportion of collisions that can overcome the activation energy for the reaction decreases as temperature increases.

  • 13. 
    According to le Châtelier’s principle if a system in equilibrium is subjected to a change in all BUT one of these conditions, there will be a tendency for a net reaction in the direction that reduces the effect of this change.
    • A. 

      Pressure

    • B. 

      Temperature

    • C. 

      Addition of a new reactant

    • D. 

      Number of moles of any component

  • 14. 
    Zn + 2HCl ---> ZnCl2 + H2 In the lab, zinc granules react fairly slowly with dilute hydrochloric acid. Which of these would MOST help to speed up the chemical reaction?
    • A. 

      Remove a catalyst

    • B. 

      Lower the temperature

    • C. 

      Use larger pieces of zinc

    • D. 

      Increase the HCL concentration

  • 15. 
    The Collision Theory explains how chemical reactions occur and why different reactions have different reaction rates. The idea behind the theory basically states thet atoms must collide in order for a chemical reaction to take place. If this theory is true, what would happen in a chemical reaction if you were to increase the concentration of HCl in the reaction: Mg + 2HCl → MgCl2 + H2
    • A. 

      The reaction would not proceed

    • B. 

      The reaction rate would increase

    • C. 

      The reaction rate would decrease

    • D. 

      There would be no change in the reaction rate

  • 16. 
    In a chemical reaction, when particle size is reduced, the rate of reaction increases because of increased surface area of the reactants. Why would increased surface area increase reaction rate?
    • A. 

      It increases the number of collisions among particles.

    • B. 

      It decreases the activation energy.

    • C. 

      It increases the concentration.

    • D. 

      It decreases the temperature.

  • 17. 
    This graph represents the energy flow of a endothermic reaction. While working on a experiment, you re-graph your results and notice that the shape of the graph is the same, but the amount of activation energy needed for the reaction to was lower. Which of these would best describe why this occurred?
    • A. 

      Additional reactants were added.

    • B. 

      A catalyst was added to the reaction.

    • C. 

      The temperature in the room was lower.

    • D. 

      There were flaws in your initial design

  • 18. 
    What MUST ALWAYS be true for a chemical reaction to occur?
    • A. 

      There must be a catalyst present.

    • B. 

      The system must be at a high temperature.

    • C. 

      The reactants’ concentrations must be high.

    • D. 

      The reactant particles must effectively collide.

  • 19. 
    Amylase becomes denatured at a temperature of 80°C. During an experiment to study the effect of varying temperature on enzyme activity, amylase's reactivity with starch was measured at body temperature (37°C), and then again at an increased temperature of 42°C. How would this increase in temperature affect the experiment?
    • A. 

      The reaction will stop

    • B. 

      The enzyme would become inactive

    • C. 

      The rate of the reaction will increase

    • D. 

      The rate of the reaction will decrease

  • 20. 
    Brad and Matt are working in the lab. They noticed that when they mixed two dilute solutions together, the reaction between them happened very slowly. Which of Matt's suggestions would BEST help to increase the rate of this reaction?
    • A. 

      Increase the concentration of both solutions

    • B. 

      Decrease the concentration of both solutions

    • C. 

      Increase the concentration of one of the solutions

    • D. 

      Decrease the concentration of one of the solutions

  • 21. 
    Based on the solubility chart, which of the listed salts is the most soluble at 25 °C?
    • A. 

      Sodium nitrate

    • B. 

      Sodium chloride

    • C. 

      Potassium nitrate

    • D. 

      Potassium chlorate

  • 22. 
    Which area of chemistry is concerned with reaction rates?
    • A. 

      Inorganic

    • B. 

      Kinetics

    • C. 

      Organic

    • D. 

      Redox

  • 23. 
    Usually, when the temperature is increased, what will happen to the rate of dissolving?
    • A. 

      It will stop.

    • B. 

      It will increase.

    • C. 

      It will decrease.

    • D. 

      It will remain the same.

  • 24. 
    Consider this reaction taking place in a closed 2 liter container:   2SO2(g) + O2(g) → 2SO3(g) If the volume of the container is decreased to 1 liter, what will happen to the equilibrium of the reaction?
    • A. 

      It will shift left.

    • B. 

      It will shift right.

    • C. 

      It will remain constant.

    • D. 

      It will decrease by half.

  • 25. 
    How do enzymes speed up chemical reactions? Enzymes
    • A. 

      Lower the activation energy of chemical reactions.

    • B. 

      Raise the temperature of the cell, speeding chemical reactions.

    • C. 

      Store ATP, allowing more energy to be used in chemical reactions

    • D. 

      Act as miniature transfer trucks gathering materials for chemical reactions, and placing them together.

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