For example, if m = 1 and n = 2, the reaction is first order in A and second order in B. The overall reaction order is simply the sum of orders for each reactant. For the example rate law here, the reaction is third order overall (1 + 2 = 3).

The integrated rate law for the first-order reaction A → products is ln[A]_t = -kt + ln[A]_0. Because this equation has the form y = mx + b, a plot of the natural log of [A] as a function of time yields a straight line.

: a chemical reaction in which the rate of reaction is proportional to the concentration of each of three reacting molecules — compare order of a reaction.

Here, the order with respect to A is given by x and order with respect to B is given by y. So the complete order of the reaction is the sum of x and y. For a third-order reaction, the order of the chemical reaction will be 3.

The order of a chemical reaction is the sum of the values x and y. A second order reaction is a reaction where x + y = 2. This can happen if one reactant is consumed at a rate proportional to the square of the reactant’s concentration (rate = k[A]2) or both reactants are consumed linearly over time (rate = k[A][B]).

These generally have the form 2A → products. A second kind of second-order reaction has a reaction rate that is proportional to the product of the concentrations of two reactants. Such reactions generally have the form A + B → products….14.6: Second-Order Reactions.

If you increase the concentration of a reactant, there will be more of the chemical present. More reactant particles moving together allow more collisions to happen and so the reaction rate is increased. The higher the concentration of reactants, the faster the rate of a reaction will be.

Pressure. If the pressure of gaseous reactants is increased, there are more reactant particles for a given volume. There will be more collisions and so the reaction rate is increased. The higher the pressure of reactants, the faster the rate of a reaction will be.

How to Improve Your Yield

1. Flame dry or oven dry flask and stirbar.
2. Use clean glassware.
3. Calculate and weigh reagent amounts accurately.
4. Purify reagents and solvents, if necessary.
5. Be sure your reactant is pure.
6. Rinse (3 times with reaction solvent) flasks and syringes used to transfer reactant and reagents.

Increasing the pressure shifts equilibrium towards the side with fewer moles of gas, so in this reaction the equilibrium will move to the right. Hence, a shift towards the right hand side will increase the yield of methanol.