The reactant in a first order reaction decreased in concentration from 0.287M to 0.115M in 44.6s. Calculate the rate constant, k, in seconds^-1.
Do I use In(0.287/0.115) = k x 44.6 ???? Or am I doing it all wrong ??
Do I use In(0.287/0.115) = k x 44.6 ???? Or am I doing it all wrong ??
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That's what you do.
Regarding your previous question about the two reactions (HCN <------> H+ + CN- etc) The reason the second reaction was reversed was simply because of the way the question was worded and the reaction you were trying to solve for. But that is why I used 10^14 instead of 10^-14. If you do need to reverse the reaction, you need to use 1/K instead of K.
Regarding your previous question about the two reactions (HCN <------> H+ + CN- etc) The reason the second reaction was reversed was simply because of the way the question was worded and the reaction you were trying to solve for. But that is why I used 10^14 instead of 10^-14. If you do need to reverse the reaction, you need to use 1/K instead of K.
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I get .0205 both ways.
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k = -ln([A]/[A0])/t = -ln(0.115/0.287)/44.6 s