Question

Oxygen and chlorine gas are mixed in a container with partial pressure of 401 mmHg and 136 mmHg Respectively. What is the total pressure inside the container?

Answer 1

Answer:

The answer is 53.2L

Explanation:

Avogadro’s Law

Avogadro’s Law, also known as the Mole-Volume Law or Volume Amount Law, states that volume (V) and moles (n) are directly proportional as long as pressure (P) and temperature (T) are held constant. This mole-volume relationship is depicted with the addition or removal of gas molecules from a closed container with a moveable piston.

Avogadro's Law (Moles & Volume)

As more and more gas molecules are pumped into the container they push up against the moveable piston and thereby increase the volume inside the container. This direct mole-volume relationship can be plotted onto a chart and provide the following:

Moles-Volume-Plot

Moles-Volume Plot

The direct relationship between the number of moles and volume at constant temperature and pressure is illustrated by the expression:

Volume-moles-Direct-Relationship

Volume & moles (Direct Relationship)

Avogadro’s Law Formula

By rearranging the Ideal Gas Law we can isolate V and n:

Avogadro-Law-Derived-Formula

Derived Formula (Avogadro's Law)

If temperature (T) and pressure (P) are held constant then the formula simplifies into:

Avogadro-Law-V/n-constant

Avogadro's Law (V/n = Constant)

Incorporating the two sets of data (2 volumes, 2 moles) produces the Avogadro’s Law formula as:

Avogadro-Law-V1n1-V2n2

Avogadro's Law (V1/n1 = V2/n2)

Answer 2

Answer:

537 mmHg is the total pressure

Explanation:

In a mixture of gases, the total pressure from the mixture is the sum of the partial pressure from each gas in the mixture.

Our mixture contains O₂ and Cl₂

Partial pressure O₂ + Partial pressure Cl₂ = Total pressure

401 mmHg + 136 mmHg = 537 mmHg

Total pressure → 537 mmHg

This is the Dalton's Law,  the total pressure of a mixture of gases is equal to the sum of the partial pressures of the gases that are contained in the mixture.