X(g) + 2 Y(g) + 2 Z(g) -->3 M(g) + 2 N(g)
I've already found the orders for the following to be: X is 2nd, Y is 1st, Z is 0 and overall of course is 3. But I am confused about the below question. I initially guess that No it doens't occur in one step..but the reasons why I am not sure and can't find in my text or lecture notes (at least not explicitly stated.
Does the reaction occur in one step? Give reasons. (Select all that apply.)
Yes.
No.
Exponents in the rate equation do not match the coefficients in the balanced equation.
Exponents in the rate equation match the coefficients in the balanced equation.
The overall order is two or greater.
The overall order is three or greater.
One of the exponents is zero.
All exponents are nonzero.
The reaction is reversible.
All reactions occur in one step.
To determine if the reaction occurs in one step, you need to compare the stoichiometric coefficients of the balanced equation to the exponents in the rate equation.
The balanced equation is: X(g) + 2 Y(g) + 2 Z(g) --> 3 M(g) + 2 N(g)
The rate equation is: rate = k[X]^a[Y]^b[Z]^c
Here, a, b, and c are the exponents, and k is the rate constant.
To check if the reaction occurs in one step, you need to compare the exponents (a, b, and c) to the stoichiometric coefficients in the balanced equation.
In this case, the exponents are not provided, so you cannot directly compare them to the coefficients in the balanced equation. Therefore, you cannot determine whether the reaction occurs in one step based on this information.
However, you can eliminate some options based on the given information:
- Exponents in the rate equation do not match the coefficients in the balanced equation: This cannot be determined without knowing the exponents.
- Exponents in the rate equation match the coefficients in the balanced equation: This cannot be determined without knowing the exponents.
- The overall order is two or greater: This is not the case as the overall order is 3.
- The overall order is three or greater: This is true, as the overall order is indeed 3.
- One of the exponents is zero: This cannot be determined without knowing the exponents.
- All exponents are nonzero: This cannot be determined without knowing the exponents.
- The reaction is reversible: This cannot be determined without additional information.
- All reactions occur in one step: This cannot be determined without additional information.
Therefore, the correct answers are:
- No
- The overall order is three or greater.
To determine whether the reaction occurs in one step or not, we need to consider the information given and the criteria for a reaction to occur in one step.
In a one-step reaction, the rate equation must match the stoichiometry of the balanced equation. This means that the exponents in the rate equation should match the coefficients in the balanced equation.
Given that the reaction is:
X(g) + 2 Y(g) + 2 Z(g) → 3 M(g) + 2 N(g)
The exponents in the rate equation should be 1 for X, 2 for Y, and 2 for Z in order to match the coefficients in the balanced equation.
Now let's analyze the options:
Yes - This response is incorrect because we have not yet determined if the exponents in the rate equation match the coefficients.
No - This response is correct because we cannot conclude that the reaction occurs in one step at this point.
Exponents in the rate equation do not match the coefficients in the balanced equation - This response is correct because we can see that the exponents in the rate equation do not match the stoichiometry of the balanced equation.
Exponents in the rate equation match the coefficients in the balanced equation - This response is incorrect because the exponents do not match the coefficients.
The overall order is two or greater - This response is incorrect because the overall order is 3, as stated in the question.
The overall order is three or greater - This response is correct, as the overall order is indeed three.
One of the exponents is zero - This response is incorrect because none of the exponents are zero.
All exponents are nonzero - This response is correct because none of the exponents in the rate equation are zero.
The reaction is reversible - This response is irrelevant to determining if the reaction occurs in one step.
All reactions occur in one step - This response is incorrect because not all reactions occur in one step.
In conclusion, the correct responses are:
- No
- Exponents in the rate equation do not match the coefficients in the balanced equation
- The overall order is three or greater
- All exponents are nonzero