Question

A:

The standard free Energy for this reaction is....
PIICK CORRECT ANSWER PLEASE
26.1 kJ
-52.1 kJ
52.1 kJ
-26.1 kJ
B:
Is this reaction spontaneous.......
no
None of the above
yes
Need more information
C l_{2}(g)+2 B r^{-}(a q) \longrightarrow 2 C l^{-}(a q)+B r_{2} C l_{2}(g)+2 e-\longrightarrow 2 C l^{-}(a q), E=1.36{~V} B r_{2}(g)+2 e-\longrightarrow 2 B r^{-}(a q), E=1.09

Answer 1

Answer and Explanation:

A: The standard free energy for this reaction is -52.1 kJ.

B: This reaction is spontaneous.

C: The given reaction involves the conversion of chlorine gas (Cl2) and bromide ions (Br-) into chloride ions (Cl-) and bromine gas (Br2) through a series of electron transfer steps. The standard reduction potentials for these steps are provided.

To determine the spontaneity of the overall reaction, we need to compare the sum of the reduction potentials (E) for the reduction half-reactions involved.

In this case, the reduction potential for the conversion of chlorine gas (Cl2) to chloride ions (Cl-) is 1.36 V, and the reduction potential for the conversion of bromine gas (Br2) to bromide ions (Br-) is 1.09 V.

Since the overall reaction involves the sum of these two reduction potentials, which results in a positive value (1.36 + 1.09 = 2.45 V), we can conclude that the reaction is spontaneous.

Therefore, the correct answer for part B is "yes."