differentiating between order reactions

[Sofi Ghasemzadeh 2G]

How do you differentiate between/classify zero, first, second, etc. order reactions?

[jennacostello8]

A zero-order reaction is independent of concentration and proceeds at a constant rate. A first-order reaction depends on the concentration of one of the reactants. A second-order reaction rate is proportional to the square of the concentration of a reactant or the product of the concentration of two reactants.

[jadyndavidson]

Another way to differentiate between the order of reactions is by the graphs of their integrated rate law. In order to do this I used the three equations given on the equation sheet and a helpful study tool I will link below. With the concentration of A vs t with a negative slope of k is shown, that is a zero-order reaction. When ln[A] vs time is shown with a negative slope of k, this is a first order reaction. When 1/[A] vs time is shown with a positive slope of k that is representative of a 2nd order rate law.

[Damin Rawlins 3B]

The order of a chemical reaction depends on the rate of the reaction with respect to the concentration of one or more reactants. A zero-order reaction has a constant rate, while a first-order reaction has a rate proportional to the concentration of a single reactant. A second-order reaction has a rate proportional to the square of the concentration of a single reactant or the product of the concentrations of two different reactants. Higher-order reactions follow similar patterns.

[Maia Hull 1H]

To determine the overall order for a reaction, you can add the order of each individual reactant that is part of the rate law. For example, if reactant A is first order, and reactant B is second order, then the overall rate of the reaction would be third order.