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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]p
Your 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!
What else can I help you with?
What has the largest value of the constant k?
how does the rate law show how concentration changes after the rate of reaction
What is k Rate kAmBn?
In the context of chemistry, "k Rate kAmBn" refers to the rate constant (k) of a reaction involving reactants A and B, where "m" and "n" represent the stoichiometric coefficients of these reactants in the rate law. The rate of the reaction can be expressed as proportional to the concentrations of A and B raised to their respective powers, leading to the equation: rate = k [A]^m [B]^n. This relationship helps in understanding how changes in concentration affect the speed of the reaction.
What is the rate of a reaction if the value of k is 0.1 is 1 M and B is 2 M?
To calculate the rate of a reaction, you typically use the rate law equation, which can be expressed as ( \text{Rate} = k[A]^m[B]^n ), where ( k ) is the rate constant, ( [A] ) and ( [B] ) are the concentrations of the reactants, and ( m ) and ( n ) are their respective orders. Assuming a simple first-order reaction with respect to both A and B (i.e., ( m = n = 1 )), the rate would be calculated as ( \text{Rate} = 0.1 \times (1)^1 \times (2)^1 = 0.2 , \text{M/s} ). Thus, the reaction rate is 0.2 M/s.
Find a formula for Poiseuilles Law given that the rate of flow is proportional to the fourth power of the radius and Use k as the proportionality constant?
Rate of flow varies as R^4 where R is the radius or Rate of flow = (k) x (R^4)
What is K in the right large reaction rate equals K a MB and?
In the expression for the reaction rate, ( K ) represents the rate constant, which is a proportionality factor that quantifies the relationship between the concentration of reactants (in this case, ( a ), ( M ), and ( B )) and the rate of the reaction. The value of ( K ) is dependent on factors such as temperature and the specific reaction mechanism. It reflects the intrinsic properties of the reaction and is essential for predicting how the reaction rate changes with varying concentrations of reactants.
What has the largest value of the constant k?
how does the rate law show how concentration changes after the rate of reaction
What is the rate of a reaction if the value of k is A and B are each 2 M?
The rate of a reaction can be determined using the rate law expression, which involves the rate constant (k) and the concentrations of reactants (A and B). Without knowing the specific form of the rate law, we cannot calculate the rate based solely on the values of the concentrations A and B. Additional information about the rate law or the order of the reaction with respect to A and B would be needed.
The concentration of both A and B was doubled the reaction rate also doubled What is the rate law for this reaction?
The rate law for this reaction is rate = k[A][B], where the rate constant k is doubled along with the concentrations of A and B.
What is the k in the rate law equation?
A rate constant
What is the rate law for a zero-order reaction?
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.
Which equation is an expression of the rate law?
Rate = k[A]m[B]n
What is the rate law for this reaction A plus 2B C plus D?
The rate law for the reaction A + 2B -> C + D is: rate = k[A][B]^2, where k is the rate constant and [A] and [B] are the concentrations of reactants A and B, respectively.
What has the largest values of the rate constant k?
how does the rate law show how concentration changes after the rate of reaction
What is the rate law expression for a first-order reaction?
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.
What is the general form of a rate law?
The general form of a rate law is rate = k[A]^m[B]^n, where rate is the reaction rate, k is the rate constant, [A] and [B] are the concentrations of reactants A and B, and m and n are the respective reaction orders for A and B.
What units must the rate constant have based on the rate law, and can you provide an example of how to calculate it?
The rate constant must have units that make the rate equation balanced. For example, if the rate law is rate kA2B, the rate constant k must have units of M-2 s-1. To calculate the rate constant, you can use experimental data and the rate law equation to solve for k.
What is the zero order reaction rate law and how does it determine the rate of a chemical reaction?
The zero order reaction rate law states that the rate of a chemical reaction is independent of the concentration of the reactants. This means that the rate of the reaction remains constant over time. The rate of the reaction is determined solely by the rate constant, which is specific to each reaction. This rate law is expressed as: Rate k, where k is the rate constant.
