The rate constant for the reaction:
`CO_(2) + overset(ɵ)(OH) rarr HCO_(3)^(ɵ)`
in the aqueous solution is `4 xx 10^(-3) L mol^(-1) s^(-1)`. The number of mole per volume of `CO_(2)` and `overset(ɵ)(OH)` are `10^(-6)` and `10^(-1) mol L^(-1)`. Also predict the mole of `HCO_(3)^(ɵ)` formed per second.

Explanation

To solve the problem, we need to determine the rate of formation of HCO3⁻ ions from the given reaction and the provided concentrations of CO2 and OH⁻ ions. Here’s a step-by-step solution:

### Step 1: Understand the Reaction
The reaction given is:
\[ \text{CO}_2 + \text{OH}^- \rightarrow \text{HCO}_3^- \]
This indicates that CO2 reacts with hydroxide ions (OH⁻) to form bicarbonate ions (HCO3⁻).

### Step 2: Identify the Rate Constant and Concentrations
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