What I know:
vol of hydrogen peroxide sample is 8.72ml
mass of hydrogen peroxide sample is 8.72g
barometric pressure in lab is 764.29 mm HG
temp in lab is 21 celcius
vol of oxygen gas collected is 99.4 mL
1) How many moles of oxygen were collected
n= .0821 x 284 divided by 1atm x 99.4 mL
n=.23 moles
that doesnt seem right :(
2) using the balanced equation (there is twice as much h202 needed as o2 produced). What is the molarity of the hydrogen peroxide solution?
It would be double my answer in #1, but i dont think that answer is right
3) what is the mass percent hydrogen peroxide if the density is 1.00g/ml
4) calculate the volume of oxygen gas that would be produced upon the decomposition of 10ml of 30%(m/m) aqueous hydrogen peroxide solution. Assume the gas is collected at 1atm and 25 degrees celcius and density of hydrogen peroxide is 1.11g/mL.
2007-11-13 07:57:48 · 2 answers · asked by shirah d 2 in Science & Mathematics ➔ Chemistry
I1) PV = nRT
n = PV/RT. I think you got it upside down.
Convert P to atm, V to L, if you are using R in L atm mol-1 K-1. ALWAYS write down the units and you won't go wrong.
2) Take number of moles in (1). Double it cos q tells you to. then use
molarity x volume (L) = number of moles.
That should get you started.
2007-11-13 11:48:12 · answer #1 · answered by Facts Matter 7 · 0⤊ 0⤋
This seems like a case of the good old M1V1= M2V2 What exactly are the "false" statements for? Do you just need to explain reasoning for your answer?
2016-04-03 23:12:22 · answer #2 · answered by Anonymous · 0⤊ 0⤋