Honors Chemistry Chapter 14 Gases Review

A set of flashcards derived from the lecture notes covering gases in chemistry, focusing on kinetic theory, gas laws, and practical calculations.

What are the key points of the kinetic molecular theory (KMT) for gases?

Gases have rapid, random motion; no attraction between particles; no volume, mostly empty space; and collisions that involve no loss of kinetic energy.

What is the general formula for the Ideal Gas Law?

$PV=nRT$ where P is pressure, V is volume, n is number of moles, R is the ideal gas constant, and T is temperature.

At what temperature do all substances have the same average kinetic energy?

At the same temperature in Kelvin.

What is the value of the ideal gas constant R in atm L/mol K?

$R = 0.0821 ext{ atm L/mol K}$.

What is the standard pressure in mm Hg?

760.0 mm Hg.

How do you convert Celsius temperature to Kelvin?

$K = °C + 273$.

What happens to lighter gases at the same temperature compared to heavier gases?

Lighter gases move faster than heavier gases.

What is Dalton's Law of Partial Pressures?

The total pressure of a gas mixture is the sum of the partial pressures of each component.

How can you calculate the density (D) of a gas?

D = rac{m}{V} where m is mass and V is volume.

What is a significant difference between ideal gases and real gases?

Real gases have intermolecular forces and occupy volume, whereas ideal gases do not.

What is the partial pressure of sulfur gas if the total pressure of a mixture is 247.6 kPa and the partial pressure of oxygen is 123.2 kPa?

124.4 kPa.

At constant temperature, if a gas occupies 250.0 mL at 800.0 mm Hg, what volume will it occupy at 20.0 mm Hg?

1.00 x 10^4 mL.

What is the internal temperature in Celsius if the pressure of a gas in a rigid container drops from 112.0 kPa to 88 kPa?

-43 °C.

What is the mass of oxygen gas in a mixture if its pressure is 123.2 kPa and occupies 1520 mL at 0 °C?

2.64 g.

If the density of a gas at STP is 0.975 g/L, what is its molar mass?

21.0 g/mol.

How do you calculate pressure in kPa from mm Hg?

Convert using the equation P ( ext{mm Hg}) imes rac{101.3 ext{ kPa}}{760.0 ext{ mm Hg}}.