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For the reaction N2(g) + 3H2(g) -> 2NH3(g), the rate of formation of NH3 is 2.5*10⁻⁴ mol L⁻¹ s⁻¹. What are the rate of disappearance of N2 and the rate of disappearance of H2 (in mol L⁻¹ s⁻¹), respectively?

1. 3.75 * 10⁻⁴, 1.25 * 10⁻⁴
2. 1.25 * 10⁻⁴, 2.5 * 10⁻⁴
3. 1.25 * 10⁻⁴, 3.75 * 10⁻⁴
4. 5.0 * 10⁻⁴, 3.75 * 10⁻⁴

Correct answer: 1.25 * 10⁻⁴, 3.75 * 10⁻⁴

Solution

Using stoichiometric ratios, rate of N2 loss = (1/2)(2.5e-4) = 1.25e-4 and rate of H2 loss = (3/2)(2.5e-4) = 3.75e-4 mol L⁻¹ s⁻¹.

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