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Q: What is the rate of a reaction if the value of k is 0.1 is 1 M and B is 2 M?

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No, 0.01 is not written as 0.01% in percent rate. 0.01 in percent rate is 1%.

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!

4,5 (mol/L)/s

1

With only one year the value is 11600

Related questions

Since the reaction is first order with respect to H2, if the concentration of H2 were halved, the rate of the reaction would be halved. This can be seen by entering one for each value in the rate equation, then changing the value of [H2] to 1/2 while keeping the other values the same: The rate changes from 1 to 1/2.

In a zero order overall process, the rate and rate constant will be the same. (Reaction order is an exponent, and if that exponent is "0" then the value is "1" and will cancel out.)

0.4 (mol/L)/s

No, 0.01 is not written as 0.01% in percent rate. 0.01 in percent rate is 1%.

Chain Reaction - 1980 1980-04-01 was released on: USA: 1 April 1980

Chain Reaction - 1980 1980-05-01 was released on: USA: 1 May 1980

A 1.5 order of reaction refers to a reaction where the rate of the reaction is directly proportional to the concentration of one reactant raised to the power of 1.5. This type of reaction does not follow typical integer orders such as first, second, or zero order reactions. The reaction rate is proportional to the square root of the concentration of the reactant.

1. The rate of forward reaction = to the rate of backward reaction. 2. Concentration of the substance are constant.

The overall reaction order for the rate law rate = k[A]^2[B][C] is 4, which is calculated by summing the individual reaction orders for each reactant ([A]^2 has an order of 2, [B] has an order of 1, [C] has an order of 1).

temperature is proportional to 1/time taken for reaction to complete (rate of reaction)

the answer is rate

equilibrium means the rate of forward reaction = rate of backward reaction... there are three types of equilibrium 1. amount of products > amount of reactants 2. amount of products = amount of reactants 3. amount of products < amount of reactants