Kinetics unit test
A test on this unit alone, marked as a percentage and a letter grade — for the test your class is actually sitting, rather than for May. Answer everything, then submit once: seeing the answer to question 3 before attempting question 4 makes the final percentage meaningless.
Activation energy
Why order cannot be read from coefficients
Reaction mechanism
Intermediate vs catalyst
Arrhenius equation
Rate law
Catalysis
Steady-state intermediates
Pseudo-first-order conditions
Energy profile diagram
Method of initial rates
Why a catalyst does not shift equilibrium
Short answer 1. Define or explain: Determining order graphically
3 ptsShort answer 2. Define or explain: Zero-order kinetics
3 ptsShort answer 3. Define or explain: Collision theory
3 ptsShort answer 4. Define or explain: Rate-determining step
3 ptsFree response
10 ptsA student measures initial-rate data at constant temperature for the decomposition 2 N₂O₅(g) → 4 NO₂(g) + O₂(g). Trial 1: [N₂O₅] = 0.010 M, rate = 4.8 × 10⁻⁶ M/s Trial 2: [N₂O₅] = 0.020 M, rate = 9.6 × 10⁻⁶ M/s The reaction has an activation energy of 103 kJ/mol.
Determine the order of the reaction with respect to N₂O₅, and write the rate law.
Calculate the rate constant k, including units.
Describe the reaction-energy diagram for this reaction, identifying what must be labeled on it.
Explain the effect of adding a catalyst on the activation energy and on the rate.