A balloon contains a mixture of 2 gases, X and Y. If the pressure in the balloon is 1.50 atm and there are 3 moles of X and 7 moles of Y present, what is the partial pressure of each gas?

Partial Pressure of X = 0.45 atm

Partial Pressure of Y = 1.05 atm

Explanation:

Mixture of gas = Gas X + Gas Y

Total number of moles = 3 + 7 = 10 moles

Total pressure = 1.50 atm

The relationship between partial pressure, total pressure and number of moles is given as;

Partial pressure of gas X  /  Total pressure = Number of moles of gas X  /  Total number of moles

Partial Pressure of gas X  / 1.50 = 3 / 10

Partial Pressure of gas X = 1.5 * 3 / 10 = 0.45 atm

The total pressure of a mixture is a sum total of the individual pressures, hence;

Pressure of mixture = Partial Pressure of X  +   Partial pressure of Y

1.5 = 0.45 +  Partial pressure of Y

Partial Pressure of Y = 1.5 - 0.45 = 1.05 atm

a. the law of proportion states the combination of 2 atoms in a specific ratio to produce multiple compounds such as the given statement of question ‘1st compound contains 88.8 % cu ’ indicates 88.8 g of cu is present along with 11.2 g oxygen in 100 g of compound whereas the statement ‘2st compound contains 79.9 % cu ’ indicates 79.9 g of cu is present along with 20.1 g oxygen in 100 g of compound

1st compound contains 88.8 g cu

for cu

m = 63 g /mol

atomic % = 88.8 /63 = 1.42

for o

m = 16 g /mol

atomic % = 11.2 /16 = 0.7

b. the emperical formula of 1st compound is

cu1.4o0.7

cu2o