AP24 Q2 Class 19 (Dalton's Law; Partial Pressure)

Front

What is Dalton's Law of Partial Pressures?

Back

Dalton's Law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas.

Front

Define partial pressure.

Back

Partial pressure is the pressure that a single gas in a mixture would exert if it occupied the entire volume alone at the same temperature.

Front

How do you calculate the total pressure of a gas mixture?

Back

Total pressure (P_total) = P_gas1 + P_gas2 + ... + P_gasN, where P_gas is the partial pressure of each gas.

Front

What is the ideal gas law equation?

Back

The ideal gas law is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.

Front

How do you convert pressure from mm Hg to atm?

Back

To convert mm Hg to atm, divide the pressure in mm Hg by 760. (P_atm = P_mmHg / 760)

Front

What is the molar mass of Cl2O7?

Back

The molar mass of Cl2O7 is approximately 162.9 g/mol.

Front

If 32.0 g of Cl2O7 decomposes, how many moles are produced?

Back

Moles of Cl2O7 = mass (g) / molar mass (g/mol) = 32.0 g / 162.9 g/mol ≈ 0.196 moles.

Front

What is the relationship between moles and pressure in a gas?

Back

At constant temperature and volume, pressure is directly proportional to the number of moles of gas (P ∝ n).

Front

How do you find the mass of a gas from its moles?

Back

Mass (g) = moles × molar mass (g/mol).

Front

What is the significance of temperature in gas laws?

Back

Temperature must be measured in Kelvin for gas law calculations, as it affects the kinetic energy and pressure of the gas.