They are experimentally determined exponents
5.4 (apex)
4.5 (mol/L)/s
The equation is M = -3N.
The equation is N = 4*M.
0.5 . . . apex
Rate = k[A]m[B]n
They are experimentally determined exponents.
r=[A]m[B]n APPLEX
The rate law equation, which is usually in the form: rate = k[A]^m[B]^n, shows how the rate of a reaction depends on the concentrations of reactants A and B. Here, k is the rate constant, [A] and [B] are the concentrations of the reactants, and m and n are the respective reaction orders.
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.
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 ).
r=[A]m[B]n APPLEX
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.
Rate= k[A]m[B]n is the formula that shows how the rate depends on the concentration of the reactants.
The rate of the reaction can be calculated using the rate law rate = k[A]^m[B]^n. Plugging in the given values: rate = 0.02*(3)^3*(3)^3 = 0.022727 = 14.58 M/s.
5.4 (apex)
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).