TG-3_Final

The dominant intermolecular forces that explain the higher boiling point of HI compared to HCl are:

• dipole-dipole

• London (Dispersión)

• Hidrogen Bond

• dipole-induced dipole

The boiling point of the following substances (CH₄, CH₃CH₂CH₃, H₂O, and H₂S) can be predicted to increase in the series:

• CH₄ > CH₃CH₂CH₃ > H₂O > H₂S

• H₂O > H₂S > CH₃CH₂CH₃ > CH₄

• H₂S > H₂O > CH₃CH₂CH₃ > CH₄

• H₂O > H₂S > CH₄ > CH₃CH₂CH₃

Explain the main reason why the boiling point of acetone (C₃H₆O) is 56 ºC, while that of 2-propanol (C₃H₈O) is 82 ºC

• 2-propanol has a higher molecular mass

• 2-propanol has a greater dipole momen

• 2-propanol forms hydrogen bonds

• acetone exhibits weak ion-dipole interactions

Which compound would you expect to have the higher boiling point, cis-dichloroethene or trans-dichloroethene

• cis-dichloroethene because the larger dipole-dipole interactions

• cis-dichloroethene because the larger London interactions

• trans-dichloroethene because the larger dipole-dipole interactions

• trans-dichloroethene because the larger London interactions

Using the ideal gas equation of state derived from the Kinetic Molecular Theory of gases, it can be stated that:

• At constant V, the pressure of a gas is directly proportional to the average velocity of its particles

• At constant V, the pressure of a gas is inversely proportional to the average velocity of its particles

• The pressure of a gas does not depend on the average velocity of the particles

• The pressure is independent of the number of gas particles

Using the Maxwell velocity distribution for the molecules of an ideal gas, it can be stated that:

• Most probable velocity > Average velocity > Root mean square velocity

• Most probable velocity > Root mean square velocity > Average velocity

• Root mean square velocity > Most probable velocity > Average velocity

• Average velocity > Most probable velocity > Root mean square velocity

The Charles's law for ideal gases is stated as:

• For a certain amount of gas at constant pressure, the gas volume is directly proportional to the temperature

• For a certain amount of gas at constant pressure, the gas volume is inversely proportional to the temperature

• For a certain amount of gas at constant temperature, the gas volume is directly proportional to the pressure

• For a certain amount of gas at constant temperature, the gas volume is inversely proportional to the pressure

What are the partial pressures of N₂, O₂ and CH₄ in a mixture where their respective molar fractions are 0.6; 0.2 and 0.2, and the total pressure is 1 atm

• P(N₂) = 0.6 atm

  P(O₂) = 0.2 atm

  P(CH₄) = 0.2 atm

• P(N₂) = 1 atm

  P(O₂) = 1 atm

  P(CH₄) = 1 atm

• P(N₂) = 0.6 atm

  P(O₂) = P(CH₄)= 0.4 atm

• P(N₂) = 1 atm

  P(O₂) = 0.2 atm

  P(CH₄) = 0.2 atm

If three balloons are filled with He, N₂, and NH₃ respectively, it can be predicted that the rate at which they deflate will vary as follows

• He > NH₃ > N₂

• NH₃ > N₂ > He

• N₂ > NH₃ > He

• He > N₂ > NH₃

The compressibility factor (Z) of a real gas:

• Is equal to 1

• Is less than 1 when it occupies more volume than it would if it behaved as an ideal gas

• Is less than 1 when it exhibits positive deviations from ideality

• Is less than 1 when the attractive forces between its molecules become significant