What does the slope equal in the graph of a zero order reaction?

In the context of zero-order reactions, the rate of the reaction is constant and does not depend on the concentration of the reactants. The rate law for a zero-order reaction can be represented as:

[ \text{Rate} = k ]

where ( k ) is the rate constant. When you plot the concentration of the reactant versus time, the graph will yield a straight line because the rate at which reactant is consumed stays the same over time.

The equation that describes a zero-order reaction can be expressed in terms of concentration ( [A] ):

[ [A] = -kt + [A]_0 ]

In this equation, ( [A]_0 ) is the initial concentration of the reactant, and as time progresses, the term ( -kt ) describes how the concentration decreases linearly with time.

When rearranging this equation into the slope-intercept form of a line, ( y = mx + b ):

• The y-intercept is the initial concentration ( [A]_0 ).
• The slope ( m ) of the line is equal to ( -k ), indicating that the slope of the graph is negative and directly proportional to the rate constant, but with a negative