Molality (m) = moles of solute / kg of solvent. Assuming 1 L of water = 1 kg, molality = 0.5 moles / 1 kg = 0.5 m.

Using Raoult's Law: P_solution = X_solvent * P_solvent. X_solvent = P_solution / P_solvent = 80/100 = 0.8, thus X_solute = 1 - X_solvent = 0.2.

Relative lowering of vapor pressure = (P° - P) / P° = (100 - 80) / 100 = 0.2.

Activation energy is the minimum energy required to initiate a chemical reaction.

For a first-order reaction, the rate is directly proportional to the concentration of reactants, so doubling the concentration doubles the rate.

For a first-order reaction, the rate is directly proportional to the concentration of the reactant, so doubling the concentration doubles the rate.

Increasing the concentration of reactants generally increases the rate of reaction due to more frequent collisions.

The correct formula is moles = mass / molar mass.

The formula for calculating the number of moles is moles = mass / molar mass.

Number of moles = Molarity x Volume (in liters).

Freezing point depression = Kf * m = 1.86 °C kg/mol * 1 mol/kg = 1.86 °C.

Molality (m) = moles of solute / kg of solvent = 3 moles / 1 kg = 3 m.

Molality (m) = moles of solute / kg of solvent = 3 moles / 0.5 kg = 6 m.

pH = -log[H+] = -log(1 x 10^-3) = 3.

All of the above factors affect the rate of a chemical reaction.

The relationship is given by ΔG = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin.

The rate of a reaction is directly proportional to the concentration of reactants raised to their respective powers in the rate law.

Standard temperature and pressure (STP) is defined as 273 K and 1 atm.

The gas constant R is commonly expressed in the unit L·atm/(K·mol).

Dissolving ammonium nitrate in water absorbs heat, making it an endothermic process.

Endothermic reactions absorb heat, feel cold, and have a positive ΔH; they do not release heat.

An ideal solution has a constant boiling point and obeys Raoult's law, while variable composition is not a characteristic.

The ideal gas constant can be represented as R = 0.0821 L·atm/(K·mol) or R = 8.314 J/(K·mol).

Exothermic reactions release heat to the surroundings, resulting in a negative enthalpy change.

Exothermic reactions release heat, resulting in a negative enthalpy change.

Ideal gases are considered to have no volume and no intermolecular forces.