What is the equation for this?
If I have two compounds, x and y, that react and form product, p, with a reaction rate of k. What is the equation way of writing this reaction out? Does MM kinetics apply here? Its not exactly enzyme and substrate. The two components can both run out.
Also, how would I go about find the rate in an experiment?
Any help would be appreciated!
Answer:
In general,
rate = k * [x]^a * [y]^b
where a and b are exponents that are the "order" of the reaction in x and y, respectively. I don't see an immediate need to invoke MM kinetics here.
You need to run several experiments in which you learn the effect of varying concentration of x and y so that you can determine these exponents. For example, if you start with a large concentration of y (excess) and then vary x from 1 to 2 to 4, and you find that the rate goes from 1 to 4 to 16, then you know a = 2.
Hi
This is relationed with the chemical equilibrium, that is explained as the state of a reaction in which the moles of the reaction dont changeand is the same to say the relative quantities of two substances or more remain constant.
If you have the reaction:
ax + by = cp with a reaction rate:
K = (P)"c/ (X)"a(Y)"b
Note.- I have troubles () is a clasp, and " is potentiation
where a, b and c represents the numbreo of moles of the reaction.
Then when you have a value of K that is the constant of equilibrium of the reaction over 1.0, This means that the reaction is favored into the products , in the other hand, if the value of K is lower than 1.0, this means in this reaction the reactives wont react at all, is the same to say the reaction wont be very efficient.
Now, this values are determined for manyreactions in labs, measuring the concentracions of productos obtained as well as the reaction continues
I recommend you to read the le chatelier principia, its very interesting and is relationed with your question
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