- #1

i_love_science

- 80

- 2

- Homework Statement:
- In an acid solution, sucrose (C12H22O11) will decompose into fructose and glucose. A plot of ln[C12H22O11] versus time gives a straight line with a slope of -0.45 hr^(-1). What is the rate law for this decomposition reaction?

- Relevant Equations:
- rate law

I think this is a first order reaction because ln[C12H22O11] vs. time is linear. The k value is the negative of the slope. Therefore, my answer is rate = 0.45 hr

The correct solution is rate = -0.45 hr

^{-1}[C12H22O11].The correct solution is rate = -0.45 hr

^{-1}[C12H22O11]^{0}. I don't understand why this is a zero order reaction, or why the k value is -0.45. Is the solution wrong? Thanks.