[Minerva]

C6H12O6 (s) + 6O2 --> 6CO2(g) + 6H2O (l)

Assuming that none of the intermmediates have appreciable concentrations, what are the values of d[C6H12O6]/dt, d[O2]/dt, d[CO2]/dt, and d[H2O]/dt, given that the overall rate is 2.4x10^-4mol/L*s.


Attempt:
-d[C6H12O6]/dt = -1/6d[O2]/dt = 1/6d[CO2]/dt = 1/6d[H2O]/dt which is the same as k[C6H12O6][O2]^6. Right? k is 2.4x10^-4 mol/Ls.

Do I have to use the product over reactant equilibrium equation? k=[CO2]^6[H2O]^6 / [glucose][O2}^6

But how am I suppose to solve it if there aren't any concentrations given?

Thank you.

[Babcock_Hall]

The units of the rate constant of a first-order reaction are (seconds)^-1.  I think that the question is ambiguous unless one more clearly defines what one means by the rate.  Is it appearance of a certain product, or is it disappearance of the reactant.