uci student

Why doesn't potassium ion K+ from KMnO4 appear in the following two unbalanced equations: MnO4– + C2O42– Mn2+ + CO2 MnO4– + Fe2+ Mn2+ + Fe3+ ? A. The presence of K+ would result in a net positive charge in the products. B. The equations cannot be balanced...

"blank" mL of 6.0 M H2SO4 are needed to prepare 300 mL of 1.0 M H2SO4 solution. its 49.8

Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction? (Cl)sub2 + 3[(F)sub2] <=> 2 [ClFsub3] i put -d(Cl2)/dt = 3[-d(F2)/dt] but apparently that isnt right, and im not quite sure why it isnt...

What is the molarity of H3O+ in a 4.97×10-2 M NH4Cl solution that hydrolyzes according to the equation. NH4+(aq) + H2O(l) = H3O+(aq) + NH3(aq)

2 mno4 16 h 5 c2o4 then 2 mn 8 h20 10 co2

answer is d. i already figured it myself, just wanted to share.

First off, yes they misspelled "wich" second. the answer is NOT EEEEE! third, the answer IS D!!! if the date on this is old, and youre from a future webworks, make sure to read the answer and not just the letter because sometimes they mix up the choices t...

first answer isnt redox, second one isnt calcium, third is for sure pb. this is difficult because it doesnt match up to reading, webworks are starting to get unreasonable.

well yea, but the only responses listed are as follows: -d(Cl2)/dt = 2[-d(F2)/dt] -d(Cl2)/dt = 3[-d(F2)/dt] 2[-d(Cl2)/dt] = -d(F2)/dt 3[-d(Cl2)/dt] = -d(F2)/dt -d(Cl2)/dt = -d(F2)/dt and none of those make sense.

-d(Cl2)/dt = 3[-d(F2)/dt] 2[-d(Cl2)/dt] = -d(F2)/dt 3[-d(Cl2)/dt] = -d(F2)/dt -d(Cl2)/dt = -d(F2)/dt

shut up lex. yes it is.

part a is iii, iv

using the table II a) i, iv b) ii, iii c) viii d) vi

the value of the forward rate constant (kf), the value of the reverse rate constant (kr), the value of the forward rate, and the value of the reverse rate