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Determine the rate of a reaction that follows the rate law rate kAmBn where k 0.2 A 3 M B 3 M m 1 n 2?
5.4 (apex)
Determine the rate of a reaction that follows the rate law rate kAmBn where k 1.5 A 1 M B 3 M m 2 n 1?
4.5 (mol/L)/s
M varies directly as N. If M-6N2What is the answer or give the equation?
The equation is M = -3N.
What is the equation for relating N to M if Abdul needs to read 4 novels each month Let N be the number of novels Abdul needs to read in M months?
The equation is N = 4*M.
What is the rate constant of a reaction if rate 1.5 molL A is 1 M B is 3 M m2 and n 1?
0.5 . . . apex
Which equation is an expression of the rate law?
Rate = k[A]m[B]n
What are m and n in the rate law equation rate kAmBn?
They are experimentally determined exponents.
What equation is an expression of the rate of law?
r=[A]m[B]n APPLEX
What equation shows how rate depends on concentrations of reactions?
The equation is called the rate law equation. For the reaction aA+bB =>cC+dD the rate law would be rate = k[A]^m[B]^n where k is the rate constant and m and n are the "order" with respect to each reactant. m and n must be determined experimentally and may or may not be the same as the coefficients a and b.
What are m and n in the rate law equation rateK(A)m(B)n?
In the rate law equation ( \text{rate} = k[A]^m[B]^n ), ( m ) and ( n ) represent the reaction orders with respect to reactants ( A ) and ( B ), respectively. These values indicate how the rate of the reaction changes in response to changes in the concentrations of the reactants. They are determined experimentally and can be whole numbers or fractions, reflecting the complexity of the reaction mechanism.
What is the rate of a reaction that follows the rate law rate kAmBn where k 0.2 A3 M B3 M m1 n2?
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.
What is k in the rate of law equation?
In the rate law equation, represented as ( \text{Rate} = k[A]^m[B]^n ), ( k ) is the rate constant that reflects the speed of the reaction at a given temperature. It is specific to the reaction and depends on factors such as temperature and the presence of catalysts. The units of ( k ) vary based on the overall order of the reaction, which is determined by the sum of the exponents ( m ) and ( n ).
Which equation would be used to calculate the rate constant from inital concentrations?
To calculate the rate constant (k) from initial concentrations, you would typically use the rate law equation for the reaction, which is expressed as ( \text{Rate} = k[A]^m[B]^n ), where ( [A] ) and ( [B] ) are the initial concentrations of the reactants, and ( m ) and ( n ) are their respective reaction orders. By measuring the initial rate of the reaction and substituting the initial concentrations into the rate law, you can rearrange the equation to solve for the rate constant ( k ).
What are m an n in the rate law eqation rate k(A)(b)?
In the rate law equation ( \text{rate} = k[A]^m[B]^n ), ( m ) and ( n ) represent the reaction orders with respect to the reactants ( A ) and ( B ), respectively. These values indicate how the reaction rate is affected by the concentrations of the reactants: ( m ) shows the sensitivity of the rate to changes in concentration of ( A ), while ( n ) does the same for ( B ). The orders are determined experimentally and can be whole numbers, fractions, or zero, depending on the reaction mechanism.
How can the rate constant be determined fro the rate law?
The rate constant can be determined from the rate law by rearranging the rate equation to isolate the rate constant (k). Typically, the rate law is expressed as ( \text{Rate} = k [A]^m [B]^n ), where ( [A] ) and ( [B] ) are the concentrations of reactants and ( m ) and ( n ) are their respective reaction orders. By measuring the reaction rate at known concentrations of the reactants, you can calculate k using the formula ( k = \frac{\text{Rate}}{[A]^m [B]^n} ). This requires experimental data to provide the necessary values for rate and concentrations.
What is the rate law for the uncatalyzed reaction?
The rate law for an uncatalyzed reaction typically depends on the reaction mechanism and the stoichiometry of the reactants involved. It is expressed in the form ( \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 the reaction orders with respect to each reactant. The specific values of ( m ) and ( n ) are determined experimentally and may not necessarily correspond to the stoichiometric coefficients in the balanced equation.
How can the rate constant be determined form the rate law?
The rate constant can be determined from the rate law by rearranging the rate equation to isolate the constant. For a reaction with a rate law of the form ( \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, one can measure the reaction rate at known concentrations. By substituting these values into the rate law and solving for ( k ), the rate constant can be calculated. This process often involves experimental data collected under controlled conditions.
