Study the chemical reaction.
A + B ⟶ C + D
A scientist studying this reaction states the reaction is first order with regard to A and zeroth order with regard to B.
What is the rate law for this reaction?
Rate = K [A]
Rate = K [B]
Rate = K [A]^2[B]
Rate = K [A][B]
Can someone walk me through this problem? I'm not sure where to start.
rate = k(A)^x(B)^y
The problem tells you that the reaction is 1st order with respect to A and zero order with respect to B. The order number is the exponent so x = 1 and y = 0
rate = k(A)^1(B)^0 = k(A)(1) = k(A)
Well, well, well, looks like we've got a chemical reaction conundrum here! Don't worry, my friend, Clown Bot is here to walk you through it with some humor sprinkled in.
Now, let's talk about rate laws. Rate laws describe how the rate of a reaction depends on the concentration of the reactants. In this case, we're given that the reaction is first order with regard to A and zeroth order with regard to B.
First order means that the rate depends on the concentration of A raised to the power of 1 (aka just [A]). Zeroth order means that the rate does not depend on the concentration of B at all. So we can chuck out the options of Rate = K [B] and Rate = K [A]^2[B].
Now, we're left with two options: Rate = K [A] and Rate = K [A][B].
Since the rate depends on A being first order, the concentration of A must be in the rate law. But since the rate does not depend on B, we can't include it in the rate law.
Therefore, the correct rate law for this reaction is... *drumroll, please*... Rate = K [A]!
I hope that explanation tickled your funny bone and helped clear things up. If you have any more questions, don't hesitate to ask!
To determine the rate law for a reaction, we need to examine the experimental data and determine how changes in the concentrations of reactants affect the rate of the reaction.
The reaction is stated to be first order with respect to A and zeroth order with respect to B. This means that the rate of the reaction is directly proportional to the concentration of A and B does not affect the rate.
Based on this information, we can conclude that the rate law for this reaction is:
Rate = K [A]^1 [B]^0.
Since any value raised to the power of zero is equal to 1, we can simplify the rate law to:
Rate = K [A].
Therefore, the correct answer is:
Rate = K [A].
Sure! Let's walk through this step-by-step.
First, let's understand what it means for a chemical reaction to be "first order" or "zeroth order" with regard to a reactant.
In a chemical reaction, the rate law describes the relationship between the concentrations of the reactants and the rate of the reaction. The general form of a rate law is:
Rate = K [A]^m [B]^n
Where Rate is the rate of the reaction, K is the rate constant, [A] and [B] are the concentrations of reactants A and B, and m and n represent the order of the reaction with respect to A and B, respectively.
If the reaction is first order with regard to a reactant, it means that the rate of the reaction is directly proportional to the concentration of that reactant. In other words, doubling the concentration of a reactant will double the rate of the reaction. Mathematically, this corresponds to m = 1.
On the other hand, if the reaction is zeroth order with regard to a reactant, it means that the concentration of that reactant does not affect the rate of the reaction. In other words, doubling or halving the concentration of a reactant will not change the rate of the reaction. Mathematically, this corresponds to m = 0.
In the given chemical reaction, the scientist states that the reaction is first order with regard to reactant A and zeroth order with regard to reactant B. Knowing this information, we can determine the rate law for the reaction.
Since the reaction is first order with regard to A, the concentration of A will be raised to the power of 1 (m = 1) in the rate law equation.
Since the reaction is zeroth order with regard to B, the concentration of B will be raised to the power of 0 (n = 0) in the rate law equation. Any value raised to the power of 0 is equal to 1, so the concentration of B does not affect the rate of the reaction.
Hence, the rate law for this reaction is:
Rate = K [A]^1 [B]^0
Simplifying further, we get:
Rate = K [A]^1 = K [A]
Therefore, the correct rate law for this reaction is:
Rate = K [A]
I hope this explanation helps! Let me know if you have any more questions.