(A)After experimentation you have determined the following rate equations:
1. Rate = k[H2] [NO]2
2. Rate = k[H2]2[O2]
3. Rate = k[H2] [NO]
Identify the order of reaction for each of these rate equations
1. The order of reaction for equation 1 is 1st order with respect to [H2] and 2nd order with respect to [NO]. The overall order of reaction is 3rd order.
2. The order of reaction for equation 2 is 2nd order with respect to [H2] and 1st order with respect to [O2]. The overall order of reaction is 3rd order.
3. The order of reaction for equation 3 is 1st order with respect to [H2] and 1st order with respect to [NO]. The overall order of reaction is 2nd order.
To identify the order of reaction for each of the given rate equations, we examine the exponents (powers) to which the concentration terms are raised.
Let's analyze each rate equation one by one:
1. Rate = k[H2] [NO]2:
In this rate equation, the exponents are 1 for [H2] and 2 for [NO]. Since the sum of the exponents for each reactant is equal to the overall order of reaction, the overall order here is 1 + 2 = 3.
Therefore, the order of reaction for this rate equation is 3.
2. Rate = k[H2]2[O2]:
In this rate equation, the exponents are 2 for [H2] and 1 for [O2]. Again, we sum up the exponents to find the overall order of reaction, which is 2 + 1 = 3.
Therefore, the order of reaction for this rate equation is 3 as well.
3. Rate = k[H2] [NO]:
In this rate equation, the exponents are 1 for [H2] and 1 for [NO]. Once again, summing up the exponents gives us the overall order of reaction, which is 1 + 1 = 2.
Therefore, the order of reaction for this rate equation is 2.
To summarize:
1. Rate = k[H2] [NO]2: The order of reaction is 3.
2. Rate = k[H2]2[O2]: The order of reaction is 3.
3. Rate = k[H2] [NO]: The order of reaction is 2.