When the numerator of any expression or fraction is zero then the result is zero because zero divided by any number is always equal to zero.
That is correct.
When the denominator is equal to zero, the expression is undefined. Close to those places, the expression tends towards plus infinity, or minus infinity. In other words, setting the denominator to zero will tell you where there are vertical asymptotes.
A zero. Zero in the denominator make the expression undefined for algebraic purposes.
You must look at the condition when the expression is greater or equal to zero and the case (condition) when it is less that zero.
The rate law for a zero-order reaction is rate k, where k is the rate constant. In a zero-order reaction, the rate of the reaction is independent of the concentration of the reactants.
In a zero-order reaction, the rate of the reaction is independent of the concentration of the reactants. The rate law for a zero-order reaction is rate k, where k is the rate constant. This means that the rate of the reaction is constant and does not change with the concentration of the reactants.
The rate constant for a zero-order reaction is a constant value that represents the rate at which the reaction proceeds, regardless of the concentration of reactants.
The rate law expression for a first-order reaction is: Rate kA, where Rate is the reaction rate, k is the rate constant, and A is the concentration of the reactant.
The zero-order rate law equation is Rate k, where k is the rate constant. In a zero-order reaction, the rate of the reaction is independent of the concentration of the reactants. This means that the rate of the reaction remains constant over time, regardless of changes in reactant concentrations.
The rate constant for a zero-order reaction is a constant value that represents the rate at which the reaction proceeds, regardless of the concentration of reactants. It is typically denoted as "k" and has units of concentration/time.
For a zero order reaction, the half-life is calculated using the equation: t1/2 = [A]0 / 2k, where [A]0 is the initial concentration of the reactant and k is the rate constant of the reaction. The half-life is independent of the initial concentration of the reactant in zero order reactions.
The order of the photoelectric reaction is zero order because the rate of the reaction does not depend on the concentration of the reactants. The rate is solely determined by the intensity of the incident light.
To determine the order of reaction from a graph, you can look at the slope of the graph. If the graph is linear and the slope is 1, the reaction is first order. If the slope is 2, the reaction is second order. If the slope is 0, the reaction is zero order.
A zero-order reaction is independent of the concentration of reactants and proceeds at a constant rate. Light can influence the rate of a zero-order reaction by providing the activation energy needed for the reaction to occur. In some cases, light can also act as a catalyst, speeding up the reaction without being consumed itself.
If the order of a reactant is zero, its concentration will not affect the rate of the reaction. This means that changes in the concentration of the reactant will not change the rate at which the reaction proceeds. The rate of the reaction will only be influenced by the factors affecting the overall rate law of the reaction.
The order of a reaction with respect to ClO2 is determined by the exponent of ClO2 in the rate law expression. If the rate law is of the form rate = k[ClO2]^n, then the order with respect to ClO2 is n. This value can be determined experimentally by measuring how changes in the concentration of ClO2 affect the reaction rate. If the concentration of ClO2 does not appear in the rate law, then the order with respect to ClO2 is zero.