The rate for a certain reaction is k = 6.00*10 -3s-1 . If the initial reactant c

Question

The rate for a certain reaction is k = 6.00*10-3s-1. If the initial reactant concentration was 0.450M, what will the concentration be after 6.00 mins? A zero-order reaction has a constant rate of 1.60*10-4M/s. if after 40.0s the concentration has dropped to1.00*10-2 M, what is the initial concentration? The rate for a certain reaction is k = 6.00*10-3s-1. If the initial reactant concentration was 0.450M, what will the concentration be after 6.00 mins? A zero-order reaction has a constant rate of 1.60*10-4M/s. if after 40.0s the concentration has dropped to1.00*10-2 M, what is the initial concentration?

Explanation / Answer

For first order reaction:                                        ln[A] = - kt + ln [A]0 Data:              k = 6.00*10-3s-1          [A]0 = 0.450 M             t  = 6.00 min                = 6 * 60 s                = 360 s Upon substituting the data in the formula,          ln[A] = -  6.00*10-3s-1*360s + ln (0.450)              = -2.16 -0.798               =- 2.958      [A]   = 0.0518M For zero order reaction:                                   [A] = - kt + [A]0                         1.00*10-2 = - 1.60*10-4M/s  * 40.0 s + [A]0                                 [A]0 = 0.0164 M                         1.00*10-2 = - 1.60*10-4M/s  * 40.0 s + [A]0                                 [A]0 = 0.0164 M      

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