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The reaction A + B -> C + D obeys the rate law r = (2 * 10⁻³ M⁻¹ s⁻¹)[A][B]. It is started with 1.0 mole each of A and B in a fixed volume of 5 litre. How many seconds are required for the moles of A to fall to 0.25?
- 7500
- 3750
- 1500
- 15000
Correct answer: 7500
Solution
Using the equal-concentration second-order integrated law, 1/0.05 - 1/0.2 = 15 = kt, giving t = 15/(2*10⁻³) = 7500 s.
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