Answer to Question #267746 in General Chemistry for jho

Question

Using the Dalton’s Law of Partial Pressure, solve the problem below.

1. O2 is prepared by decomposing calcium chlorate (Ca(ClO3)2) and collecting 255 ml sample over water at 40℃ and a total pressure of 798 mmHg. What is the partial pressure of O2? What is the mass of the O2 collected?

Need a complete solution

Answer 1

Using the Dalton's law

P (Total) = Poxygen +Pwater

The vapor pressure of water is 21mmHg

751mmHg = Poxygen + 21 mmHg

Poxygen = 751 mmHg - 21 mmHg

Poxygen =730 mmHg

Convert the partial pressure of oxygen in to atmosphere

(730 mmHg) (1 atm / 760 mmHg) = 0.96 atm