Question

Consider the reaction: A + B → products

The following rate law was experimentally determined: rate =
k[A][B]^{2}

If the concentration of A stays the same and B doubles, the rate
will

increase by a factor of sixteen.

triple.

quadruple.

double.

Which statement is correct?

The exponents in the rate law NEVER match the coefficients in the
balanced chemical reaction.

The exponents in the rate law MUST be determined by
experiment.

The exponents in the rate law ALWAYS match the coefficients in the
balanced chemical reaction.

The initial rate method is being used to study the kinetics of a
particular reaction. The absorbance for the reaction is being
monitored as a function of time. The table here contains absorbance
vs time data.

time, s | 0 | 4 | 8 | 12 | 16 | 20 |
---|---|---|---|---|---|---|

Abs | 0.11 | 0.13 | 0.15 | 0.17 | 0.19 | 0.21 |

What is the initial rate for this reaction?

Initial Rate = Abs/s

Answer #1

The reaction A→B has been experimentally determined to be second
order. The initial rate is 0.0100M/s at an initial concentration of
A of 0.150 M .
1. What is the initial rate at [A]=0.850 M ?
a.
0.321 M/s
b.
0.113 M/s
c.
5.67×10−2 M/s

The experimentally determined rate law for the reaction
2NO(g)+2H2(g)→N2(g)+2H2O(g) is
rate=k[NO]2[H2].
Part A
What are the reaction orders in this rate law?
Enter your answers numerically separated by commas.
nNO, nH2 =
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Part B
Would the reaction rate increase more if we double the
concentration of NO or the concentration of H2?
A) The reaction rate will increase more if we double the
concentration of NO.
B) The reaction rate will increase more if we double the...

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