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.
Answer:
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[tex]H_{rxn}[/tex] = ∑ Bond Energy ( reactants) - ∑ Bond Energy (products)
= [ (2 × C=O) + (2 × C=S) ] - [ (2 × C=O) + ( 2 × C=S) ]
we know that;
Δ[tex]H_{rxn}[/tex] = -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)[tex]_{reactant}[/tex] - ( 2 × C=S)[tex]_{product}[/tex]
-3.85 kJ/mole = (2 × C=S)[tex]_{reactant}[/tex] - ( 2 × 552 kJ/mole)
(2 × C=S)[tex]_{reactant}[/tex] = -3.85 kJ/mole + 1104 kJ /mole
(2 × C=S)[tex]_{reactant}[/tex] = 1100.15 kJ/mole
2 × ( C=S)[tex]_{reactant}[/tex] = 1100.15 kJ/mole
( C=S)[tex]_{reactant}[/tex] = 1100.15 kJ/mole / 2
( C=S)[tex]_{reactant}[/tex] = 550.1 kJ/mole
Therefore, the apparent bond energy of a carbon–sulfur bond is 550.1 kJ/mole
The apparent bond energy of a carbon-sulfur bond in COS is equal to 550.08 kJ/mol.
Given the following data:
Scientific data:
To determine the apparent bond energy of a carbon-sulfur bond in COS:
First of all, we would write a balanced chemical equation for the chemical reaction as follows:
[tex]2COS \rightarrow CO_2 + CS_2[/tex]
The enthalpy change of two (2) moles of COS is:
[tex]\Delta H_{rxn} = -3.2 \times 10^{-24}\times 2 \times 6.02 \times 10^{23}\\\\\Delta H_{rxn} =-3.85\;kJ/mol.[/tex]
Mathematically, the enthalpy change of a chemical reaction is given by this equation:
[tex]\Delta H_{rxn} = \sum Bond\;Energy_{(reactansts)} - \sum Bond\;Energy_{(products)}\\\\\Delta H_{rxn} = [(2\times C=O)+ (2\times C=S)]- [(2\times C=O)+ (2\times C=S)][/tex]
Substituting the parameters into the equation, we have;
[tex]-3.85 = (2\times C=S)- [2\times 552]\\\\(2\times C=S)=1104-3.85\\\\(2\times C=S)=1100.15\\\\(C=S)=\frac{1100.15}{2} \\\\(C=S)=550.08\;kJ/mol[/tex]
Therefore, the apparent bond energy of a carbon-sulfur bond in COS is equal to 550.08 kJ/mol.
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Complete Question:
The enthalpy change for the reaction between two molecules of carbon oxysulfide (COS) to form one molecule of [tex]CO_2[/tex] and one molecule of [tex]CS_2[/tex], as shown below, is [tex]-3.2 \times 10^{-24}[/tex] 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.]
