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Formula Recall Deck
Flashcards for key formulas.
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Synthesize kinetics concepts, rate laws, and Arrhenius calculations across the entire chapter.
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Flashcards for key formulas.
Final check of chapter capabilities.
Progressive difficulty MCQs spanning the chapter.
A chemical reaction has a measured rate constant ( k = 2.3 \times 10^{-5} \text{ L mol}^{-1} \text{ s}^{-1} ). What is the order of this reaction?
Calculate age using first-order decay.
An archaeological artifact containing wood had only 80% of the ( ^{14}\text{C} ) found in a living tree. The half-life (( t_{1/2} )) of ( ^{14}\text{C} ) is 5730 years. Follow the steps below to estimate the age of the sample.
List the initial concentration percentage, final concentration percentage, and half-life.
Provide the formula to find the rate constant (k), and the first-order integrated rate law for time (t).
Substitute your known values into the formulas.
Show the intermediate calculation steps, including finding k first.
State the final estimated age with appropriate units.
Calculate Ea from tabulated data.
The rate constant for the decomposition of ( \text{N}_2\text{O}_5 ) is ( 1.70 \times 10^{-5} \text{ s}^{-1} ) at ( 20^\circ\text{C} ) and ( 25.7 \times 10^{-5} \text{ s}^{-1} ) at ( 40^\circ\text{C} ). Calculate the activation energy (( E_a )) in J/mol. (Use ( R = 8.314 \text{ J K}^{-1} \text{mol}^{-1} )).
List k1, k2, and convert both temperatures to Kelvin.
State the two-temperature form of the Arrhenius equation.
Plug in all known values into the equation.
Show the calculation for log(k2/k1) and the temperature term, then isolate Ea.
Provide the final Activation Energy in J/mol (or kJ/mol).