ok here goes :'( i cant seem to handle this question, help asap as in any second after i post this would be rather impressive:

 

calculate the mass of KClO3 required to produce 1.00dm3 (at 20 degrees C and 101.3 kPa) of oxygen.

 

molar gas volume = 24000 cm3 mol-1 at 20 degrees C and 101.31 kPa

 

does it have anythin to do with PV=nRT seriously im well confused i have the answer HOWEVER i dont understand how it has been achieved. *sigh*

please!!! come on!

PV=nRT is the way to go. i assume you have the reaction equation as well

indeed i do:

 

2KClO3 --> 2KCl + 302

 

ok, so what after pv=nrt do you rearrange that to n=pv/rt:confused:

indeed i do:

 

2KClO3 --> 2KCl + 302

 

ok, so what after pv=nrt do you rearrange that to n=pv/rt:confused:

 

Correct. This will give you the mass of oxygen that the specified reaction conditions will generate. In conjunction with the reaction equation specified above, you'll then be able to figure out the number of moles of oxygen produced and from that the number of moles of KClO3 produced. Once you have the number of moles, the calculation of actual mass is pretty easy.