AP Chemistry
5.6 Reaction Energy Profile
5.3 Concentration Changes Over Time
A student studies the first-order decomposition of reactant \(\text{A}\) at two temperatures. The student obtains the following data.
For the calculations, use \(R=8.31\ \text{J mol}^{-1}\text{K}^{-1}\), \(\ln 2=0.693\), and \(\ln 20=3.00\). What is the estimated activation energy, \(E_a\), for the decomposition?
| \(T\) | \(t\) | \([\text{A}]\) |
|---|---|---|
| \(300\ \text{K}\) | \(0\ \text{s}\) | \(0.100\ \text{M}\) |
| \(300\ \text{K}\) | \(3465\ \text{s}\) | \(0.0500\ \text{M}\) |
| \(330\ \text{K}\) | \(0\ \text{s}\) | \(0.100\ \text{M}\) |
| \(330\ \text{K}\) | \(346.5\ \text{s}\) | \(0.0250\ \text{M}\) |
For the calculations, use \(R=8.31\ \text{J mol}^{-1}\text{K}^{-1}\), \(\ln 2=0.693\), and \(\ln 20=3.00\). What is the estimated activation energy, \(E_a\), for the decomposition?
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