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Postby RRahimtoola1I » Sat Mar 07, 2020 9:48 pm

How do you do this problem or other problems similar to this when they give you only the initial concentration of the reactant and then a later concentration of a product?

For the first-order reaction A > 3B + C, when initial concentration of A = 0.015 mol/L, the concentration of B increases to 0.018 mol/L in 3.0 min. (a) What is the rate constant for the reaction expressed as the rate of loss of A? (b) How much more time would be needed for the concentration of B to increase to 0.030 mol/L?

Adam Kramer 1A
Posts: 103
Joined: Sat Aug 24, 2019 12:15 am

Re: 7B.9

Postby Adam Kramer 1A » Sat Mar 07, 2020 10:00 pm

You know that B increased . 018M in 3 minutes, so A decreased by 0.06M in the same time. You can then calculate the rate and you know it's first order, so you can then plug in the variables into the rate law equation and solve for the k rate constant.

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