0.5
The rate constant is not indicative of the order of the reaction. To determine the order of the reaction, experimental data (such as concentration vs. rate data) is needed. The order of the reaction can be found by examining how changes in reactant concentrations affect the rate of the reaction.
4,5 (mol/L)/s
0.5 Apex
The correct units for a second order rate constant are M^-1 * s^-1 or L/mol * s. These units represent the concentration change over time for a second-order reaction.
8.3*10^-4
The rate constant include all parameters ((but not concentration) affecting the rate of a chemical reaction.The expression "specific reaction rate" is used when the molar concentration of reactants is a unit.
The standard units used to measure the rate constant in a chemical reaction, known as kc units, are typically expressed in moles per liter per second (mol/L/s).
You can use the Arrhenius equation to solve for the activation energy barrier (Ea). The formula is k = A * exp(-Ea/RT), where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy barrier, R is the gas constant, and T is the temperature in Kelvin. Since the rate constant triples when the temperature increases from 22.0 to 34.0, you can set up two equations using the Arrhenius equation and solve for Ea.
The rate law for this reaction is rate = k[A]^m[B]^n. From the given information, substituting the values for rate, [A], [B], and the exponents m and n, you can solve for the rate constant k. In this case, k = rate / ([A]^m[B]^n), so k = 2 / (10^2 * 3^1).
.72 (mol/L)/s
Here it is in two forms: k = A exp (-Ea/RT) ln k = ln A - Ea/RT The latter is a linearized version. In both cases... k is the rate constant, A is the frequency factor (an experimentally determined quantity related to the probability that a collision will lead to a reaction), Ea is the activation energy, R is the Universal Gas constant (8.31 J/mol K), and T is the temperature in Kelvins.
24 (mol/L)s