Based on your experimentally determined rate law for the reaction of crystal vio

Question

Based on your experimentally determined rate law for the reaction of crystal violet and OH^-, how would doubling the concentration of crystal violet affect the reaction rate? Would you have determined an identical rate law for the reaction of crystal violet and OH^-, if you had used [OH^-] of 0.030M and 0.040M instead of the concentrations you did use in the Procedure? Briefly explain. The rate law for a certain reaction is second order with respect to one of the reactants, R. Suppose study this reaction, observing the absorbance of light at the analytical wavelength for R, and n the data with respect to elapsed time. Also suppose that the concentrations of all the other reaction are in large excess, and that R is the only colored species involved. Explain which absorb In A, or 1/ A, would yield a straight-line graph when plotted against elapsed

Explanation / Answer

I need you to provide your experimental rate reaction and concentration of reactants used to determine the rate law. In theory, and as we are talking of a first order reaction, it could be done, cause the rate constant should remain the same.

However, the best way to know that, is replacing the values of concentratios given in this part, and determine the new rate law for this reaction. When you do that, you'll know if it's identical or if there's any kind of change. So replace the values obtained and see what's the result.

Hope this little information guides you and helps you.

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