How many liters of O2 gas measured at 807 torr and 250.0°C are formed by the decomposition of 253 g of KClO? (Hint: You will need a balanced equation where KClO is the reactant. The other product is KCl.)

balanced equation: 2KClO --> 2KCl + O2

conversions: the temp becomes 523
the pressure (torr) becomes 1.20

work: 253g KClO (1mol KClO/ 90.55g KClO) (1mol O2/2mol KClO)= 1.397
PV=nRT... and you want to find volume so it becomes V= nRT/P
(1.397mol) (.0821) (523K)/ 1.20atm= 49.98

how is this wrong...

1/16/2008 10:41:50 PM

atm = 760 torr

807/760 = 1.06

[Edited on January 16, 2008 at 10:47 PM. Reason : .]

1/16/2008 10:46:51 PM

i swear i always do stupid mistakes.
thanks

1/16/2008 11:01:11 PM

anyone else remember that equation by saying "pivnert"?

1/17/2008 12:02:47 AM

i've never heard of that...

1/17/2008 12:10:42 AM

this isn't really a webassign question, but I'm pretty sure its a ch201 question:

I have 900 mL of a sample at 10.51 pH, and it is neutralized with 30.62 mL of HCl at 0.1 Normality. If I were to neutralize the sample with H2SO4 instead of HCl, what volume of H2SO4 would I need.

Now If I use the Na x Va = Nb x Vb formula, and assume the H2SO4 also has a 0.1 Normality, the result I'm getting is that I need 30.62 mL of the H2SO4. Is this right? Am I using the formula correctly (if its even applicable)?

I haven't done this kind of chemistry in like 6 years...

1/21/2008 2:52:34 PM

CHEATER ALERT!!!!

1/21/2008 4:00:29 PM

^ i hope your not talkin bout me /c that is not cheating...

1/22/2008 1:25:26 AM

arpatel, not sure if you still need this info, but you have to think about normality not molarity. Sulfuric acid is diprotic while HCl is monoprotic, so the amount of mL will not be the same for both HCl and H2S04. I don't know if I can help more without giving the answer.

1/24/2008 7:49:02 PM