How does adding a chemical catalyst accelerate the rate of a chemical reaction?
Answer and explanation
Correct answer: C. Providing an alternative reaction pathway with a lower activation energy
A catalyst lowers the activation energy (Ea) for both forward and reverse reactions by providing an alternate mechanism, thereby increasing the rate constant k (Arrhenius equation) without changing Delta H, Delta G, or the equilibrium constant Keq.
Practise more Chemical Thermodynamics, Kinetics, and Equilibrium.
Free questions with an explanation for every one, and full timed Medical University Entrance Examination (Bulgaria) mock tests.
More Chemical Thermodynamics, Kinetics, and Equilibrium questions
- What thermodynamic criterion determines whether a chemical process is spontaneous at constant temperature and pressure?
- Under which thermodynamic conditions is a chemical reaction spontaneous at all temperatures?
- What are the units of the rate constant (k) for a second-order chemical reaction?
- If doubling the concentration of reactant A quadruples the initial rate of reaction, what is the reaction order with respect to A?
- According to the Arrhenius equation (k = A * e^(-Ea / RT)), what graph yields a straight line whose slope equals -Ea / R?
- For the exothermic Haber process reaction: N2(g) + 3 H2(g) <=> 2 NH3(g) (Delta H = -92 kJ/mol), how will increasing the total pressure at co…