How would you find rate order, given these concentrations and initial rates?

asked by @llians1 • 6 months ago • Chemistry • 5 pts

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2 answers

Hi Lilian! To find the order, you need to first start with a reactant. If you're looking for the order of reactant A, you want to pick two experiments that have different concentrations of A, but the same concentrations for B. You could pick Experiments 1 and 2 for that. Then, you can use an equation: enter image description here

Plug in the rates for each experiment as well as the concentrations of A for each experiment (Conc. of A from Exp. 2 on top and Conc. of A from Exp 1 on the bottom). solve for X. (Remember that the left side turns into (A2/A1)^x when you simplify).

Once you solve, the value of X represents the order of Reactant A. Then, do the same thing for B and C: enter image description here

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You can also check out this link, which has tons of examples on calculating order: https://www.clutchprep.com/chemistry/rate-law/6838/learn/2812

Hope this helps! Let us know if you have any other questions :)

answered by @sabrina • 6 months ago

The rate equation will be r=k [A]2[C} The order with respect to reactant A is second order, to reactant B is zero order and for reactant C is first order. Here's the solutions: Order for reactant A for reactant B for reactant C

From reactant B you can see that the rate does not change after multiply by 1.5*square. this shows that the rate of the reaction does not depend on the concentration of reactant B.

hope that this get to help you!

answered by @wongchiaqic1 • 6 months ago