[billsauce]

consider the reaction:
3A + B + C ---> products, rate = k[A]^2(B)[C], where the initial concentrations are as follows
[A]o = 1.0x10^-4M, (B)o=[C]o=1.00M
a) After 3 minutes, [A] = 3.26E-5M. Calculate K.
b) Calculate the half life of reaction.
c) calculate the concentration of C after 10.0 min.
d) calculate the concentration of A after 10.0 min.

So i am thinking this is psuedo 2nd order reaction because the concentration of A is much lower than B and C initially, so I know how to do a, b, and d (using integrated 2nd order rate laws)

BUT
how do i do C???