- #1
Pengwuino
Gold Member
- 5,123
- 20
So here's the problem I am faced with... dum dum dummmm
So first I figured that there will be 30.6g of hydrogen peroxide. Then I figured that there are 0.4498 moles of O2. Then using the ideal gas law...
V=nRT/P
I got ((0.4498)(0.08206)(27+273.15))/(746/760) = 11.3 Liters of O2
But supposedly I am wrong. Where did I go so horribly horribly wrong?
Oops, and i just punched in 22.6 Liters and it says I'm right... so where did I divide by 2 where I shouldn't have?
Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe):
2H2O2(aq) ---> 2H2O(l) + O2(g)
What volume of pure O2(g), collected at 27 °C and 746 torr, would be generated by decomposition of 61.2 g of a 50.0 % by mass hydrogen peroxide solution? Ignore any water vapor that may be present.
So first I figured that there will be 30.6g of hydrogen peroxide. Then I figured that there are 0.4498 moles of O2. Then using the ideal gas law...
V=nRT/P
I got ((0.4498)(0.08206)(27+273.15))/(746/760) = 11.3 Liters of O2
But supposedly I am wrong. Where did I go so horribly horribly wrong?
Oops, and i just punched in 22.6 Liters and it says I'm right... so where did I divide by 2 where I shouldn't have?
Last edited: