Characterize EACH of the three given statements as being TRUE or FALSE and then indicate the collective true-false status of the statements using the choices: (1) Both dipole-dipole interactions and hydrogen bonds are stronger than most single covalent bonds.
(2) The value of the ideal gas constant is the same for all gases under ordinary conditions of P, V, and T.
(3) Both condensation and freezing are endothermic changes of state.
A) All three statements are true.
B) Two of the three statements are true.
C) Only one of the statements is true.
D) None of the statements is true.

Question

Quizplus · Accepted Answer

- Statement 1 is FALSE because both dipole-dipole interactions and hydrogen bonds are generally weaker than most single covalent bonds. Covalent bonds involve the sharing of electrons between atoms, leading to a much stronger bond compared to the intermolecular forces of dipole-dipole interactions and hydrogen bonds.- Statement 2 is TRUE. The ideal gas constant, R, is indeed the same for all gases under ordinary conditions of pressure (P), volume (V), and temperature (T). It is a universal constant in the equation PV=nRT, where n is the number of moles of the gas.- Statement 3 is FALSE because condensation (gas to liquid) and freezing (liquid to solid) are exothermic processes, where heat is released as the substance moves to a state of lower energy.

Characterize EACH of the Three Given Statements as Being TRUE