Answer:
ΔH rxn = -1010 kJ/molC₂H₂
Explanation:
To obtain the enthalpy change for a reaction from bond energies what we do is to make an inventory of the bonds broken and formed for the balanced chemical reaction:
C₂H₂ + 5/2O₂ ⇒ 2CO₂ + H₂O
Bond Broken Bonds Formed
2 C-H + 1 C≡C + 5/2 O=O 4C=O + 2 H-O
Enthalpy bonds broken:
2 mol (456 kJ/mol)+ 1 mol (962 kJ/mol) + 5/2 mol (499 kJ/mol) = 3121.5 kJ
Enthalpy bond formed:
4 mol (802 kJ/mol) + 2 mol (462 kJ/mol) = 4132.0 kJ
ΔH rxn = H broken - H formed = 3121.5 kJ - 4132.0 kJ = - 1010 kJ (per mol C₂H₂ )
due to there reactive rate?
The basic substances are called elements
The material on the right is a darker shade than the one on the left. Also the one on the right also is less of a block and a little more shagged
Answer:
C) 2CO + O₂ → 2CO₂
Explanation:
The equation C is correct.
2CO + O₂ → 2CO₂
This equation have four oxygen atom and two carbon atoms on both side of equation. So it is correctly balanced.
All others are incorrect:
A) CO + O₂ → CO₂
this is incorrect because there are three oxygen atoms on left while two atoms on right.
B) CO + 2O₂ → 2CO₂
this is incorrect because there are five oxygen atoms on left while four atoms on right.
D) 2CO + 2O₂ → 2CO₂
this is incorrect because there are six oxygen atoms on left while four atoms on right.
