Rate Law: Methanol and ethyl acetate react to form ester and glycerol.
What is the order of reaction with respect to methanol and ethyl acetate, and what is the overall order of reactions? Please explain how to find if the answer is order 1 for methanol and order 0 for ethyl acetate.
You must have some data such as rate of reaction, concentration of reactants, etc. Without that we're in the dark.
You can always go to the web and Google that reaction. That will likely tell you the order of each and the overall order; however, it is not likely to tell you how those results were obtained. You might try a search such as "calculation of order for methanol and ethyl acetate using concentration data"
Good luck.
To determine the order of a reaction with respect to each reactant and the overall order of the reaction, you need to analyze the rate equation or rate law for the reaction. The rate law expresses the relationship between the rate of the reaction and the concentrations of the reactants.
The general form of a rate law for a reaction can be written as:
Rate = k[A]^m[B]^n
In this particular case, we need to determine the order of reaction with respect to methanol (CH3OH) and ethyl acetate (CH3COOC2H5), and the overall order of the reaction.
To find the order of the reaction with respect to methanol, you can perform experiments where you vary the initial concentration of methanol while keeping the concentration of ethyl acetate constant. Let's say you run three experiments with different initial concentrations of methanol: [CH3OH]1, [CH3OH]2, and [CH3OH]3.
From the rate equation, we can write the ratio of rates for these experiments as:
Rate1/Rate2 = ([CH3OH]1)^m / ([CH3OH]2)^m
However, as we want to determine the order of methanol (m), we can assume that m is a constant and cancel it out from the equation. This leaves us with:
Rate1/Rate2 = ([CH3OH]1) / ([CH3OH]2)
Similarly, we can compare the rates of the first and third experiments to obtain:
Rate1/Rate3 = ([CH3OH]1) / ([CH3OH]3)
If we divide these two equations, the m cancels out:
(Rate1/Rate2) / (Rate1/Rate3) = ([CH3OH]1 / [CH3OH]2) / ([CH3OH]1 / [CH3OH]3)
Rate3/Rate2 = ([CH3OH]3 / [CH3OH]2)
If the rate ratios are equal for different initial concentrations of methanol, then the order of the reaction with respect to methanol is 1 (first order). If the rate ratios are not equal, you would need to analyze the trend and potentially perform additional experiments to determine the correct order.
You can follow a similar process to determine the order of the reaction with respect to ethyl acetate (CH3COOC2H5) by keeping the concentration of methanol constant and varying the initial concentration of ethyl acetate.
Lastly, the overall order of the reaction is the sum of the orders with respect to each reactant. For example, if the order of the reaction with respect to methanol is 1 and the order with respect to ethyl acetate is 0, then the overall order of the reaction would be 1+0 = 1.