The rate constant for a zero order reaction A B + C is 6.0 10⁻³ molL ⁻¹ ~s ⁻¹ . What would be the time taken for the initial concentration of A to decrease from 0.2 M to 0.024 M ?

Step-by-step solution

For a zero order reaction, the integrated rate equation is given by [A]_t = [A]₀ - kt , where [A]₀ is the initial concentration, [A]_t is the concentration at time t , and k is the rate constant. Given values are [A]₀ = 0.2 M , [A]_t = 0.024 M , and k = 6.0 10⁻³ mol L ⁻¹ s ⁻¹ . Rearranging the equation to solve for t : t = [A]₀ - [A]_t k Substituting the values: t = 0.2 - 0.024 6.0 10⁻³ t = 0.176 6.0 10⁻³ t = 176 6 s t = 29.333... s Rounding to two decimal places, t = 29.33 s . Answer: 29.33 s