Question
What volume of oxygen gas can be collected
at 1.26 atm pressure and 2.00◦C when 39.7 g
of KClO3 decompose by heating, according to
the following equation?
2 KClO3(s) ∆/MnO2 −−−−→ 2 KCl(s) + 3 O2(g)
Answer in units of L.
at 1.26 atm pressure and 2.00◦C when 39.7 g
of KClO3 decompose by heating, according to
the following equation?
2 KClO3(s) ∆/MnO2 −−−−→ 2 KCl(s) + 3 O2(g)
Answer in units of L.
Answers
DrBob222
See your other post above but this one is not eligible for the shortcut.
Convert g KClO3 to mols. mols = g/molar mass = ?
Then convert mols KClO3 to mols O2
Use PV = nRT and convert mols CO2 to L CO2 at the conditions listed.
Convert g KClO3 to mols. mols = g/molar mass = ?
Then convert mols KClO3 to mols O2
Use PV = nRT and convert mols CO2 to L CO2 at the conditions listed.