ayam Posted December 26, 2006 Share Posted December 26, 2006 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* Link to comment Share on other sites More sharing options...
ayam Posted December 26, 2006 Author Share Posted December 26, 2006 please!!! come on! Link to comment Share on other sites More sharing options...
insane_alien Posted December 26, 2006 Share Posted December 26, 2006 PV=nRT is the way to go. i assume you have the reaction equation as well Link to comment Share on other sites More sharing options...
ayam Posted December 26, 2006 Author Share Posted December 26, 2006 indeed i do: 2KClO3 --> 2KCl + 302 ok, so what after pv=nrt do you rearrange that to n=pv/rt:confused: Link to comment Share on other sites More sharing options...
jdurg Posted December 27, 2006 Share Posted December 27, 2006 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. Link to comment Share on other sites More sharing options...
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