What will be the initial rate of a reaction if its rate constant is `10^(-3) min^(-1)` and the concentration of reactant is `0.2 mol dm^(-3)` ? How much of reactant will be converted into Products in `200 min`?

Explanation

Since `k` has unit in `min^(-1)`, thus, the given reaction is of first order.
Now, rate `= k["Concentration"]^(1)`
Rate `= 10^(-3) xx[0.2]^(1) = 2 xx 10^(-4) mol dm^(-3) min^(-1)`
Also `k = (2.303)/(200) log.(100)/((100-x))`
`x = 18.12%`