A graph of experimental data is a straight line when ln[H2] is plotted versus time. Which rate law fits the data?

A. Rate = k(ln[H2])
B. Rate = k/[H2]
C. Rate = k[H2]
D. Rate = k[H2]2

I think A as it fits the constant for a straight line. what do you think?

C. Rate = k[H2]

Just took the quiz

Yes, you are correct. When the natural logarithm of the concentration of H2 ([H2]) is plotted against time and the resulting graph is a straight line, the rate law that fits the data is A. Rate = k(ln[H2]). This suggests that the reaction rate is directly proportional to the natural logarithm of the concentration of H2.

To determine which rate law fits the given experimental data, we need to analyze the relationship between the concentration of H2 ([H2]) and the rate of the reaction.

In the given scenario, when the natural logarithm of the H2 concentration (ln[H2]) is plotted against time, a straight line is obtained. This implies that the rate of the reaction is directly proportional to the natural logarithm of the H2 concentration.

The rate law equation represents how the rate of a reaction depends on the concentration of the reactants. Based on the information provided, the rate law that fits the data would be:

A. Rate = k(ln[H2])

This rate law suggests that the rate of the reaction is proportional to the natural logarithm of the concentration of H2.

Therefore, your initial choice of option A is correct.

http://www.chem.purdue.edu/gchelp/howtosolveit/Kinetics/IntegratedRateLaws.html