2KClO3(s) 2KCl(s) + 3O2(g) If 7.17 g of KClO3 decompose and the oxygen gas is colleted in a 2.84 L glass bottle at a temperature of 23.4°C, then what would be its pressure?

Question

2KClO3(s)  2KCl(s) + 3O2(g)  If 7.17 g of KClO3 decompose and the oxygen gas is colleted in a 2.84 L glass bottle at a temperature of 23.4°C, then what would be its pressure?

aaronq · Answer

convert that mass to moles
use the coefficients to build a ratio to find moles of O2

use PV=nRT

aaronq · Answer

solve for P

anonymous · Answer

but im confused on how to convert the mass of that to moles

aaronq · Answer

moles=mass/molar mass

you can find molar masses on the periodic table

anonymous · Answer

so am i suppose to solve for oxygen because i already tried it and got it wrong.

aaronq · Answer

you're supposed to find the moles of oxygen produced then find the pressure using the ideal gas law

aaronq · Answer

making sure you use the correct gas constant, and correct units for temperature and volume