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Question:

If the rate of decomposition of N2O5 during a certain time interval is 2.4 × 10⁻⁸ molL⁻¹min⁻¹. N2O5 → 2NO2 + 1/2O2 What is the rate of formation of NO2 and O2 molL⁻¹min⁻¹?

2.3 × 10⁻⁹ and 1.2 × 10⁻⁹ respectively

3.8 × 10⁻⁸ and 0.6 × 10⁻⁸ respectively

2.4 × 10⁻⁸ and 1.5 × 10⁻⁸ respectively

4.8 × 10⁻⁸ and 1.2 × 10⁻⁸ respectively

Solution:

Rate of reaction = -d[N2O5]/dt = +1/2d[NO2]/dt = +2d[O2]/dt
Rate of formation of NO2 = d[NO2]/dt = 2(-d[N2O5]/dt) = 4.8 × 10⁻⁸ mol L⁻¹ min⁻¹
Rate of formation of O2 = d[O2]/dt = 1/2(-d[N2O5]/dt) = 1.2 × 10⁻⁸ mol L⁻¹ min⁻¹