Which of the following statements is true? a. state functions do not depend on the path taken to arrive at a particular state. b. energy is neither created nor destroyed, excluding nuclear reactions. c. delta hrxr can be determined using constant pressure calorimetry. d. delta erxp can be determined using constant volume calorimetry. e. all of the above are true.

E. All of the above are true.

Explanation:

Which of the following statements is TRUE?

A. State functions do not depend on the path taken to arrive at a particular state. TRUE. State functions like enthalpy (ΔH) and internal energy (ΔE) do not depend on the trajectory, but on the initial and final state.

B. Energy is neither created nor destroyed, excluding nuclear reactions. TRUE. Only in nuclear reactions can energy (E) can be transformed in matter (m) and vice-versa according to Einstein equation: E = m . c² (c is the speed of light).

C. ΔHrx can be determined using constant pressure calorimetry. TRUE. The enthalpy of reaction is the heat involved at constant pressure.

D. ΔErx can be determined using constant volume calorimetry. TRUE. The internal energy of reaction is the heat involved at constant volume.

intermolecular forces are the forces between molecules or particles.

there are two kinds of van der waals forces: weak london dispersion forces and stronger dipole-dipole forces.

in molecule of water there are dipole-dipole forces between negatively charged oxygen from one molecule of water and positively charger hydrogen of another molecule of water.

hydrogen bond is an electrostatic attraction between two polar groups that occurs when a hydrogen atom (h), covalently bound to a highly electronegative atom such as flourine (f), oxygen (o) and nitrogen (n) atoms.