What is the apparent bond energy of a carbon–sulfur bond in cos?

This question is incomplete, the complete question is;

The enthalpy change for the reaction between two molecules of carbon oxysulfide (COS) to form one molecule of CO₂ and one molecule of CS₂, as shown below, is -3.2 x 10⁻²⁴ kJ per molecule of COS.

The bond energy for the C-S bond in C=S has been determined to be 552 kJ/mol.

What is the apparent bond energy of a carbon-sulfur bond in COS?

NOTE: A C=O bond adjacent to another double bond is not the same as a C=O bond that is not adjacent to another double bond.  

The apparent bond energy of a carbon–sulfur bond is 550.1 kJ/mole

Explanation:

Given the data in the question and the figure 8.122 in the image below;

the given reaction can be written as follows;

2COS -----→ CO₂ + CS₂

Δ = ∑ Bond Energy ( reactants) - ∑ Bond Energy (products)

= [ (2 × C=O) + (2 × C=S) ] - [ (2 × C=O) + ( 2 × C=S) ]

we know that;

Δ  = -3.2 x 10⁻²⁴ kJ per molecule

= -3.2 x 10⁻²⁴ kJ × 2 × 6.023 × 10²³ kJ/mole

= -3.85 kJ/mole

Hence;

-3.85 kJ/mole = (2 × C=S) - ( 2 × C=S)

-3.85 kJ/mole = (2 × C=S) - ( 2 × 552 kJ/mole)

(2 × C=S) = -3.85 kJ/mole + 1104 kJ /mole

(2 × C=S)  = 1100.15 kJ/mole

2 × ( C=S) = 1100.15 kJ/mole

( C=S) = 1100.15 kJ/mole / 2

( C=S) = 550.1 kJ/mole

Therefore, the apparent bond energy of a carbon–sulfur bond is 550.1 kJ/mole

particle   p is an electron and particle q is a neutron

the answer is 1260

you spend 7 hours in school for 1 school day with 5 school days in 1 school week with 36 school weeks in a school year.

7*5*36= 1260 it's all about multiplying