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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!
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What has the largest value of the constant k?
how does the rate law show how concentration changes after the rate of reaction
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 a example of unit rate?
meters grams like K H D M D C M m is meters the unit rate for measuring the unit rate is like the middle value
What is the decimal value of the ASCII letter K?
The ASCII value of capital K is 75. For a small k it is 107.
What is the k constant in Charles law?
V/T=k
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
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 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 is the rate of a reaction if the value of k is 3 and A and B are each 2M?
If the rate law for the reaction is given by rate = k[A]^m[B]^n, where m and n are the orders of the reactants A and B, respectively, then the rate of the reaction would be calculated as rate = k[A][B]. Plugging in the values given (k = 3, A = 2M, B = 2M), the rate of the reaction would be 3*(2)*(2) = 12 M/s.
What is the rate reaction if the value of k is 0.01 a is 2 m and b is 3 m rate m a 3 b 2?
.72 (mol/L)/s
What would happen to the rate of a reaction with rate law rate k NO H2 if the concentrations of NO were doubled?
The rate would be four times larger
What has the largest value of the rate constant?
how does the rate law show how concentration changes after the rate of reaction
