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Quizzes > Science > Chemistry

Rate of Reaction Quiz: Test Your Chemistry Skills!

Ready for a chemistry reaction quiz? Dive into kinetics and test reaction rates!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art of test tubes beakers and gears on coral background promoting free reaction rates and kinetics quiz

Are you ready to tackle the ultimate rate of reaction quiz and see how far your chemistry skills reach? Our free chemistry reaction quiz challenges you with real-world scenarios, reaction rate questions, kinetics quiz puzzles, and hands-on problems that test reaction rates and reinforce core principles. You'll dive into activation energy, collision theory, and the influence of catalysts, temperature, and concentration. Whether you're aiming for top exam marks or exploring molecular magic, this quiz has you covered. After finishing, continue with our chemical equilibrium quiz or explore an organic chemistry quiz for extra practice. Let's ignite your curiosity - start now!

What does the rate of a chemical reaction measure?
The total amount of energy released
The change in concentration of reactants per unit time
The change in temperature per unit time
The change in concentration of products per unit time
The rate of a chemical reaction is defined as the change in concentration of reactants or products per unit time. It is most commonly measured by how fast reactants disappear. Knowing this rate helps chemists understand reaction kinetics. For more details, see Chemguide.
Which factor does NOT affect the rate of a reaction under typical conditions?
Color of reactants
Concentration of reactants
Temperature
Surface area of solid reactants
Reaction rates depend on factors such as temperature, concentration, surface area, and catalysts. The color of the reactants does not influence how often or how energyfully molecules collide. Color is purely a visual property and does not affect kinetic energy or collision frequency. More on factors affecting rates can be found at LibreTexts.
What happens to the average kinetic energy of molecules when temperature increases?
It decreases
It remains constant
It first decreases then increases
It increases
The kinetic molecular theory states that temperature is directly proportional to the average kinetic energy of molecules. As temperature rises, molecules move faster on average. This increased motion leads to more frequent and energetic collisions. See more at Khan Academy.
In collision theory, which condition is NOT required for a successful reaction?
Collisions must occur at the surface of a catalyst
Collisions must have enough energy
Particles must be in the correct orientation
Particles must collide
Collision theory requires that reacting species collide with sufficient energy and proper orientation to form products. A catalyst surface may help guide orientation but is not a general requirement for every reaction. Reactions can occur in homogeneous phases without any catalytic surface. More is explained at Chemguide.
What is the activation energy of a reaction?
The total energy released during the reaction
The energy difference between reactants and products
The minimum energy required for reactant molecules to form products
The energy of the transition state minus the products
Activation energy is the minimum threshold energy that reacting molecules must possess to reach the transition state and form products. It represents the height of the energy barrier. Lower activation energy means more particles can react at a given temperature. See Chemguide for more details.
How does adding a catalyst affect the rate of a reaction?
It changes the reaction equilibrium constant
It increases the activation energy
It decreases the activation energy
It increases the temperature
A catalyst provides an alternative reaction pathway with a lower activation energy, which increases the reaction rate. It does not alter the temperature or the equilibrium constant. Catalysts remain unchanged at the end of the reaction. Further explanation can be found at Khan Academy.
For a reaction with rate law rate = k [A]^2 [B], what happens to the rate when the concentration of A doubles (with [B] constant)?
It remains the same
It quadruples
It doubles
It increases eightfold
The rate law shows rate ? [A]^2, so if [A] doubles, the rate increases by 2^2 = 4 times. Since [B] stays constant, only the change in [A] affects the rate. This quadratic dependence is characteristic of second-order behavior in A. More examples are at LibreTexts.
For a first-order reaction, how does the half-life relate to the initial concentration?
Half-life depends on the activation energy
Half-life is inversely proportional to initial concentration
Half-life is independent of initial concentration
Half-life is directly proportional to initial concentration
A first-order reaction has a constant half-life given by t?/? = ln(2)/k, which does not depend on the starting concentration. This unique feature differentiates first-order kinetics from other orders. The half-life remains the same no matter how much reactant you begin with. See Chemguide for more information.
In an Arrhenius plot of ln(k) versus 1/T, what is the slope equal to?
Ea/R
-R/Ea
-Ea/R
R/Ea
The Arrhenius equation can be written as ln(k) = ln(A) - Ea/(R·T), so plotting ln(k) against 1/T yields a straight line with slope -Ea/R. This linear form is commonly used to determine activation energies experimentally. A more detailed derivation is available at LibreTexts.
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Study Outcomes

  1. Understand collision theory -

    Describe how particle collisions and activation energy determine the rate of reaction in chemical systems.

  2. Analyze temperature and concentration effects -

    Predict how changes in temperature or reactant concentration influence reaction rates using kinetics principles.

  3. Evaluate catalysts and inhibitors -

    Assess how catalysts accelerate reactions and how inhibitors slow them down without being consumed.

  4. Apply rate laws and rate constants -

    Use rate equations to calculate reaction rates and determine rate constants from experimental data.

  5. Interpret reaction kinetics data -

    Read and analyze graphs or tables to infer reaction mechanisms and identify rate-determining steps.

  6. Differentiate reaction orders -

    Distinguish zero-, first-, and second-order reactions by examining how rate changes with concentration.

Cheat Sheet

  1. Collision Theory Essentials -

    Collision theory explains that reaction rate increases when more effective collisions occur between reactant molecules; for a successful collision, particles must collide with enough energy (≥Ea) and correct orientation. In your rate of reaction quiz, remember that higher concentration and temperature boost collision frequency, enhancing reaction speed. A handy mnemonic is "E for Energy, O for Orientation" to recall both criteria.

  2. Rate Law and Reaction Order -

    The rate law expresses the reaction rate as rate = k [A]^m [B]^n, where m and n (orders) are determined experimentally, not from stoichiometry. Practice determining the rate constant k and reaction order by analyzing initial-rate data in reaction rate questions. Universities like MIT provide excellent worked examples for deducing m and n from rate vs concentration tables.

  3. Arrhenius Equation and Temperature Effects -

    The Arrhenius equation, k = A·e^( - Ea/RT), quantifies how temperature (T) influences the rate constant (k); a small increase in T can dramatically raise k by lowering the exponential barrier. For your kinetics quiz, plot ln k versus 1/T to find Ea from the slope ( - Ea/R). Remember the phrase "Ape Eats Ripe Tomatoes" to recall Arrhenius, Ea, R, Temperature.

  4. Catalysts and Alternative Pathways -

    Catalysts speed reactions by providing a lower-energy pathway without being consumed; enzymes and industrial catalysts like Fe in Haber process are prime examples. When tackling chemistry reaction quiz items, identify how catalysts alter Ea and the mechanism's transition state. Reputable sources such as the Royal Society of Chemistry detail step-by-step catalytic cycles to deepen your understanding.

  5. Impact of Concentration, Surface Area & Pressure -

    In heterogenous reactions, increasing surface area of solids (e.g., powdered vs. chunk metal) ramps up collision sites, boosting rate. For gases, Le Chatelier's principle shows that higher pressure shifts equilibria and often speeds reactions by compressing molecules closer. When you test reaction rates, compare how doubling [A] or halving particle size influences the observed rate.

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