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it tells how much the reaction rate is affected by concentration
how does the rate law show how concentration changes after the rate of reaction
K is known as the rate coefficient, or the rate constant. The value of k is particular, and varies from reaction to reaction. It is dependent on different factors such as temperature, pressure, concentration, solvent, presence of a catalyst, etc., and therefore a change in any of these gives you a new value for k. To determine the value of k, you must use the experimental data to determine if you have a zeroth order, first order, or second order reaction. As indicated by the equation below, you must also have the actual rate.Rate= k[A]m[B]n[C]pYour overall reaction order is given by the sum of the orders of reactant.If you have a zeroth order reaction overall, then k will be equal to the rate. So if the reactants are consumed at a rate of 1.00 mol/liter/sec, then your k has a value of 1.00 mol/liter/sec. This means that no matter how much of the species you add, a lot or just enough, you will not change the rate.If you have a first order reaction where the concentration of A, [A] (in mols/liter), is consumed at a rate of .004 mol/liter/sec, then k = [A]/.004 mol/liter/sec, as given by the above equation: You divide the rate by the concentrations of the reactants. The units for a first order reaction are sec-1 or 1/sec, because you are dividing moles per liter by moles per liter per second. So the concentration of this does matter. The concentration of the reactant is proportional to the rate of reaction.If you have a second order reaction, then the addition of a reactant will increase the rate of reaction by a square of the concentration of the reactant. This is because you are now dividing the rate of reaction by, for example, [HNO3]2. Remember the the previous variables m, n, or p are the experimentally determined order of reactant. So a second order reaction results in squaring the concentration. Hope that helps!
It follows from the cyclical symmetry of the cosine rule.
In order to bring the system to equilibrium, action and reaction cancel out. The resultant is the reaction.
5.4 (apex)
4.5 (mol/L)/s
The rate of the reaction can be calculated using the rate law rate = k[A]^m[B]^n. Plugging in the given values: rate = 0.02*(3)^3*(3)^3 = 0.022727 = 14.58 M/s.
They are experimentally determined exponents.
The rate of the reaction can be calculated using the rate law equation rate = k[A]^m[B]^n. Plugging in the given values k = 0.2, m = 1, n = 2, [A] = 3 M, and [B] = 3 M into the equation gives rate = 0.2 * (3)^1 * (3)^2 = 16.2 M/s.
The rate law uses the concentrations of reactants to determine the rate of a reaction. By experimentally determining the relationship between the rate of reaction and the concentrations of reactants, we can derive the rate law equation for that specific reaction.
The rate of a reaction is calculated using the concentrations of reactants.
To determine the rate of a reaction using the rate law, you need to know the rate constant (k), the concentrations of the reactants, and the order of the reaction with respect to each reactant. The rate law equation relates the rate of the reaction to these factors.
The rate of a reaction is calculated using the concentrations of reactants.
The rate law is an equation that relates the rate of a chemical reaction to the concentration of reactants. It provides information on how the rate of the reaction is influenced by the concentrations of reactants and any catalysts involved. Additionally, the rate law helps determine the specific reaction order for each reactant.
How the concentration of the reactants affects the rate of a reaction
The rate law equation relates the rate of a reaction to the concentrations of reactants. By examining the exponents of the concentrations in the rate law, one can determine how changes in the concentration of reactants affect the rate of the reaction. For example, if the exponent of a certain reactant is 2, doubling its concentration would quadruple the rate of the reaction according to the rate law equation.