Question

I only have two more attempts left and I need help on my homework. I am so lost in Chemistry right now, and I need someone to explain this in a simple way so I will not only get an A in the homework, but also in the class.

http://njit.mrooms.net/file.php/16756/Images_Chem_126_RH_/kinetics_13-18.jpg

1. Calculate the average rate of reaction between 0.0 and 47.0 s (units mol/L/s).

2.Calculate the initial rate of reaction (units mol/L/s).

3.Calculate the instantaneous rate of formation of ethylene at 46.0 s (units mol/L/s).

I tried these, but I keep getting them wrong

Answer 1

it depends on the type of reaction you have:
If A -> P
\(\Delta rate_{rxn}=\dfrac{\Delta [P]}{\Delta T}\)

Answer 2

yeah I did that. It is the change in concentration again over time right? You can choose any two points on the graph to get the avg rate of change right? but I keep getting it wrong. This is the actual reaction Cyclobutane can decompose to form ethylene: C4H8(g) → 2C2H4(g).

Answer 3

i would choose the first and last points, not just any points. (unless it's a linear relationship).