The bond enthalpy of the Br–Cl bond is equal to DH° for the reaction

BrCl(g)-> Br(g) + Cl(g).
Use the following data to find the bond enthalpy of the Br–Cl bond.

Br2(l)--->Br2(g) ÄH=30.91 KJ/mol
Br2(g)--->2Br2(g) ÄH=192.9 KJ/mol
Cl2(g)---->2Cl(g) ÄH=243.4 KJ/mol
Br2(l)+Cl2(g)-->2BrCl(g) ÄH=29.2KJ/mol

A. 219.0 kJ/mol
B. 203.5 kJ/mol
C. 14.6 kJ/mol
D. 438.0 kJ/mol
E. 407.0 kJ/mol

To find the bond enthalpy of the Br–Cl bond, we can use the concept of Hess's Law. Hess's Law states that the enthalpy change for a reaction is independent of the pathway taken and depends only on the initial and final states.

First, we need to cancel out any compounds that appear on both sides of the reaction equation. In this case, the Br2(l) appears on both sides, so we can cancel it out:

Br2(l) + Cl2(g) --> 2BrCl(g)

Next, we need to examine the given reactions and align them properly in order to cancel out any compounds that appear on both sides. Let's look at the given reactions:

1. Br2(l) ---> Br2(g) ΔH = 30.91 kJ/mol
2. Br2(g) ---> 2Br(g) ΔH = 192.9 kJ/mol
3. Cl2(g) ---> 2Cl(g) ΔH = 243.4 kJ/mol
4. Br2(l) + Cl2(g) ---> 2BrCl(g) ΔH = 29.2 kJ/mol

Now, let's align the reactions and assign appropriate coefficients to match the desired reaction:

Br2(l) ---> Br2(g) ΔH = 30.91 kJ/mol
2Br(g) + Cl2(g) ---> 2BrCl(g) ΔH = ?
2Br(g) + Cl2(g) ---> 2BrCl(g) ΔH = 29.2 kJ/mol

Since the given reactions 2 and 4 have the same reactants and products, we can subtract ΔH4 from ΔH2 to find the value of ΔH for the desired reaction:

ΔH2 - ΔH4 = 30.91 kJ/mol - 29.2 kJ/mol
= 1.71 kJ/mol

Now, we need to consider the coefficients. Since the reaction we want to find has a coefficient of 1 for BrCl(g), while the reaction we subtracted has a coefficient of 2, we need to divide the ΔH by 2:

ΔH for 2Br(g) + Cl2(g) ---> 2BrCl(g) = 1.71 kJ/mol / 2
= 0.855 kJ/mol

Finally, to find the bond enthalpy of the Br–Cl bond, we divide the ΔH by 2 (since we want the enthalpy change per mole of Br–Cl bonds):

Bond enthalpy of Br–Cl bond = 0.855 kJ/mol / 2
= 0.4285 kJ/mol

Rounding this value to the nearest whole number, the bond enthalpy of the Br–Cl bond is approximately 0.43 kJ/mol.

None of the given answer choices match this value. It's possible that there was an error made during the calculation or data input.