Graham and Dalton's Law

Dalton's Law states...

• that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.
• that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases
• how gases tend to expand when heated
• that the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.

Which equation represents Dalton's Law?

• e=mc2
• PV=nRT
• P1/T1=P2/T2
• Ptotal=P1, P2, P3...

Dalton's law of...

• Partial Pressure
• Thermodynamics
• Ideal Gas
• Physics

A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?

• 234 mmHg
• 1.37 mmHg
• 2.64 mmHg
• 1, 494 mmHg

A container holds a mixture of two different gases. The oxygen in a container exerts 80 mmHg of pressure on the inside of the container. The total pressure inside the container is 120 mmHg. What is the pressure of the other gas in the container?

• 200 mmHg

• 80 mmHg

• 40 mmHg

• 120 mmHg

A container holds three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 2.00 atm, 3.00 atm, and 4.00 atm, respectively. What is the total pressure inside the container?

• 900 atm

• 0.90 atm

• 9.00 atm

• 920 atm

how many times faster does He effuse compared to N₂ (He = 4  N₂ = 28)

• 1.2 times faster
• 2.65 times faster
• 7 times faster
• 0.377 times faster

why would O₂ effuse faster than CO₂ in the same room

• because it has more energy
• because it has a greater molar mass
• because oxygen has a higher temperature
• they will effuse the same because the temperature is fixed

what is the rate of effusion for NH₃ (M=17) if the rate of effusion for SO₂ (M=17) is 0.800m/s

• 1.55 m/s
• 2.00 m/s
• 0.500m/s
• 0.800m/s

Grahams law of effusion states that The rate of effusion of gases at the same temperature and pressure are;

• directly proportional to the mass
• inversely proportional to the molar mass
• inversely proportional to the square root of the molar mass 
• directly proportional to the square root of the molar mass