Question

Bond Dissociation Energy Suppose there is an element X which occurs naturally as X2(g). X2(g) + 2O2(g) ? X2O4(g) X2O4 has a structure X—X ?H°f of O(g) is 249 kJ/mol ?H°f of X(g) is 470.5 kJ/mol ?H°f of X2O4(g) is 33 kJ/mol The X-X single bond energy is 118 kJ/mol Use the above data to estimate the average X?O bond energy in X2O4. Give your answer to the nearest 1 kJ/mol.

          Bond Dissociation Energy

Suppose there is an element X which occurs naturally as X2(g).

X2(g) + 2O2(g) ? X2O4(g)

X2O4 has a structure X—X

?H°f of O(g) is 249 kJ/mol
?H°f of X(g) is 470.5 kJ/mol
?H°f of X2O4(g) is 33 kJ/mol
The X-X single bond energy is 118 kJ/mol

Use the above data to estimate the average X?O bond energy in X2O4.
Give your answer to the nearest 1 kJ/mol.

Bond Dissociation Energy

Suppose there is an element X which occurs naturally as X2(g).

X2(g) + 2O2(g) ? X2O4(g)

X2O4 has a structure X—X

?H°f of O(g) is 249 kJ/mol
?H°f of X(g) is 470.5 kJ/mol
?H°f of X2O4(g) is 33 kJ/mol
The X-X single bond energy is 118 kJ/mol

Use the above data to estimate the average X?O bond energy in X2O4.
Give your answer to the nearest 1 kJ/mol.

Added by Jennifer A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

08/29/2023

Step 1

This is given by the formula ΔHf = ΔHf(products) - ΔHf(reactants). For the reactants, we have 2 moles of X and 2 moles of O2. So, ΔHf(reactants) = 2*ΔHf(X) + 2*ΔHf(O2) = 2*470.5 + 2*249 = 1439 kJ/mol. For the product, we have 1 mole of X2O4. So, ΔHf(product) = Show more…

Show all steps

Thanks for your feedback!

Bond Dissociation Energy Suppose there is an element X which occurs naturally as X2(g). X2(g) + 2O2(g) → X2O4(g) X2O4 has a structure ΔH°f of O(g) is 249 kJ/mol ΔH°f of X(g) is 470.5 kJ/mol ΔH°f of X2O4(g) is 33 kJ/mol The X-X single bond energy is 118 kJ/mol Use the above data to estimate the average X⌇O bond energy in X2O4. Give your answer to the nearest 1 kJ/mol.