Chemistry MP3CP2 Review

Front

What is the kinetic-molecular theory of gases?

Back

The kinetic-molecular theory of gases explains that gas particles are in constant motion, collide elastically, and the temperature of a gas is proportional to the average kinetic energy of its particles.

Front

What is the percent composition of a compound?

Back

The percent composition of a compound is the percentage by mass of each element in the compound, calculated by dividing the mass of the element by the total mass of the compound and multiplying by 100.

Front

How do you identify limiting and excess reactants in a chemical reaction?

Back

The limiting reactant is the substance that is completely consumed first in a reaction, limiting the amount of product formed. The excess reactant is the substance that remains after the reaction.

Front

What is the formula for calculating percent yield?

Back

Percent yield = (actual yield / theoretical yield) x 100.

Front

How do you calculate the theoretical yield of a reaction?

Back

The theoretical yield is calculated based on the stoichiometry of the balanced chemical equation, using the amount of limiting reactant.

Front

What is the molar mass of BaCl2?

Back

The molar mass of BaCl2 (Barium Chloride) is approximately 137.33 g/mol (Ba) + 2 x 35.45 g/mol (Cl) = 208.23 g/mol.

Front

How do you convert grams to moles?

Back

To convert grams to moles, divide the mass of the substance (in grams) by its molar mass (in g/mol).

Front

What is the significance of the average kinetic energy in gases?

Back

The average kinetic energy of gas particles is directly related to the temperature of the gas; higher temperatures mean higher average kinetic energy.

Front

What is an elastic collision in the context of gas particles?

Back

An elastic collision is one in which there is no net loss of total kinetic energy in the system; gas particles collide without losing energy.

Front

What is the role of temperature in gas behavior?

Back

Temperature affects the speed of gas particles; as temperature increases, the particles move faster, leading to increased pressure if volume is constant.