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What else can I help you with?
What equation is an expression of the rate of law?
r=[A]m[B]n APPLEX
LThe rate of change in the equation y = m + b is represented by the m?
True
What is the part of the slope intercept form that represents the rate of change?
y=mx +b is the equation for slope intercept form. y = the output of the equation m = the slope x = the input into the formula b = the y-intercept The slope represents the rate of change. This is because for every input, or x, you put into the equation, is changed by m. So the M portion of this equation would be the rate of change.
What is the rate of a reaction if the value of k is 0.1 is 1 M and B is 2 M?
To calculate the rate of a reaction, you typically use the rate law equation, which can be expressed as ( \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. Assuming a simple first-order reaction with respect to both A and B (i.e., ( m = n = 1 )), the rate would be calculated as ( \text{Rate} = 0.1 \times (1)^1 \times (2)^1 = 0.2 , \text{M/s} ). Thus, the reaction rate is 0.2 M/s.
What does m represent in your equation?
If you are talking about linear graphs, m refers to the gradient (aka slope or rate of change).
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 are m and n in the rate law equation?
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 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.
Determine the rate of a reaction that follows the rate law RatekAmBn where K110-2 A2M B3M m2 n1?
To determine the rate of the reaction following the rate law ( \text{Rate} = k[A]^m[B]^n ), we can substitute the given values. With ( k = 1 \times 10^{-2} , \text{m}^2/\text{s} ), ( m = 2 ), and ( n = 1 ), the rate becomes ( \text{Rate} = (1 \times 10^{-2})[A]^2[B]^1 ). Thus, the reaction rate is proportional to the square of the concentration of ( A ) and directly proportional to the concentration of ( B ). The specific rate will depend on the actual concentrations of ( A ) and ( B ) used in the reaction.
What units must the rate constant have based on the rate law, and can you provide an example of how to calculate it?
The rate constant must have units that make the rate equation balanced. For example, if the rate law is rate kA2B, the rate constant k must have units of M-2 s-1. To calculate the rate constant, you can use experimental data and the rate law equation to solve for k.
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 ).
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.
What is the rate of a reaction if the value of k is 0.01 A is 2 M and B is 3 M Rate kA3B2?
The rate of the reaction is calculated using the rate equation: rate = k[A]^3[B]^2. Given k = 0.01, [A] = 2 M, and [B] = 3 M, the rate can be determined by substituting these values into the rate equation and solving for the rate.
LThe rate of change in the equation y = m + b is represented by the m?
True
