Answer to Question #172336 in General Chemistry for Dayera

Question

With steps please..

2KClO₃(s)2KCl(s) + 3O₂(g)

In an experiment, the O₂ gas formed is collected over water in a flask where the total pressure is 635 mm Hg and the temperature is 18.0°C, at which temperature the vapor pressure of water is 16 mm Hg.

(1) What is the partial pressure of O₂ in the flask? ........mm Hg

(2) If the wet O₂ gas occupies a volume of 10.33 L, how many moles of O₂ are formed?........  mol

Answer 1

1.$P_{oxygen} =(635-16)=619mm Hg$

2.$7.69×10^{-4}mol$