When the reaction begins, a $1.00\,\text{dm}^3$ solution contains $0.300\,\text{mol}$ of ethanol. By $100\,\text{s}$ the concentration of the ethanol has fallen to $0.296\,\text{mol dm}^{-3}$. What is the rate of reaction during the first $100\,\text{s}$?
- A$2.96 \times 10^{-3}\,\text{mol dm}^{-3}\,\text{s}^{-1}$
- B$3.00 \times 10^{-5}\,\text{mol dm}^{-3}\,\text{s}^{-1}$
- C$4.00 \times 10^{-5}\,\text{mol dm}^{-3}\,\text{s}^{-1}$
- D$8.00 \times 10^{-5}\,\text{mol dm}^{-3}\,\text{s}^{-1}$