Answer to Question #278551 in General Chemistry for roro chuchu

Question

4. A 3.50 g of solid CO2 isplaced in a 4.00 L container at a temperature of 300 K. When all

the solid CO2 becomes gas, what will be the pressure in the container?

1. You are task to collect gases such as N2, O2, CO2, and Ar gas. The partial pressures of N2,

O2, and CO2 are 515 torr, 215 torr, and 98 torr respectively. What is the partial pressure of

Ar, if the total pressure is 715 torr?

2. The partial pressure of N2 in a mixture of gases where the total pressure is 1.00 atm

is 400 torr. What is the mole fraction of N2?

3. A mixture of air which consists of 26% oxygen, 68% nitrogen, and 6 % traces gases

at a 1 atmospheric pressure. Use those percentages to compute for the individual

pressure of each gas at STP applying Dalton`s law of partial pressures.

4. A mixture of 25.0 g oxygen and 65.0 g of helium used by deep-sea diver has a total

pressure of 5 atm. What will be the partial pressure of each gas?

Answer 1

Use ideal gas equation

PV =nRT

given V= 4.00l

mass m = 600g 

number of mols = 600g/44.01 g/mol 

T=300 k

P =nRT/V 

= 600g* 0.0821 l atm/mol.k * 300 K/4.00 l *44.01 g/mol  

 = 83.9 atm

Answer

pressure = 83.9 atm