Integrated rate equations: zero, first, second order
Chemical Kinetics · Chemistry
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A first-order reaction has k = 0.02 s⁻¹, [A]₀ = 0.8 M. Find [A] after 60 s. Step 1: ln[A] = ln[A]₀ − kt = ln(0.8) − 0.02 × 60. Step 2: ln(0.8) = −0.223; kt = 1.2. Step 3: ln[A] = −0.223 − 1.2 = −1.423. Step 4: [A] = e^(−1.423) = 0.241 M. First order: equal time fractions, equal concentration fractions.