Question

The above reaction was studied at 300 K by monitoring the concentration of FeSO₄, in which initial concentration was 10 M and after half an hour became 8.8 M. The rate of production of Fe₂(SO₄)₃ is _____ × 10⁻⁶ mol L⁻¹ s⁻¹

Hint:

The rate of production of a product in a reaction can be calculated by determining the rate of change of concentration of a reactant and using stoichiometric ratios.

Answer 1

Correct Answer: 333

Rate of reaction is given by the change in concentration of FeSO₄: \[ \frac{-\Delta [FeSO₄]}{\Delta t} \] Substitute the given values: \[ \frac{-10 + 8.8}{30 \times 60} = \frac{1.2}{1800} = 6.67 \times 10^{-4} \] From the given reaction, the rate of production of Fe₂(SO₄)₃ is related to the rate of FeSO₄: \[ \frac{1}{6} \times \frac{-\Delta [FeSO₄]}{\Delta t} \] Substitute the value of \(\frac{-\Delta [FeSO₄]}{\Delta t}\): \[ \text{Rate of production of Fe}_2(SO₄)_3 = \frac{3}{6} \times 6.67 \times 10^{-4} = 333.33 \times 10^{-6} \] Thus, the rate of production of Fe₂(SO₄)₃ is \(333 \times 10^{-6}\) mol L⁻¹ s⁻¹. Hence,