Question

Calculate the energy change in kJ/mol for the reaction Li(g) + F(g) => Li+(g) + F-(g) (separated ions) using the following information: Li(g) => Li+(g) + e- +520 kJ/mol, F(g) + e- => F-(g) -328 kJ/mol. Enter your answer as the closest whole number with the appropriate sign and without units.

Options:
A) -192
B) 192
C) 520
D) -848

Answer 1

The energy change in kJ/mol for the reaction Li(g) + F(g) => Li+(g) + F-(g) (separated ions) is 192 kJ/mol.

Step-by-step explanation:

To calculate the energy change in kJ/mol for the reaction Li(g) + F(g) => Li+(g) + F-(g) (separated ions), we need to consider the energy changes for the individual steps involved in the reaction.

Given the information provided, we know that the ionization energy of Li(g) is +520 kJ/mol, and the electron affinity for F(g) is -328 kJ/mol.

Since the reaction involves the transfer of one electron from Li(g) to F(g), the energy change can be calculated by summing up the ionization energy of Li(g) and the electron affinity of F(g).

Therefore, the energy change in kJ/mol for this reaction is (-328 + 520) kJ/mol, which is equal to 192 kJ/mol.