Bond Enthalpy

Using the table of average bond energies below the image, the ΔH for the reaction in kJ is.....

• + 160 kJ
• -63 kJ
• - 160 kJ
• -217 kJ

Using the reaction & table above, determine the change in energy and whether or not the reaction is endothermic or exothermic:

• -2054 kJ endothermic

• 2023 kJ endothermic

• -2023 kJ exothermic

• 2023 kJ exothermic

How much energy is required to break all of the bonds in the first molecule depicted in the reaction above? (you must include the proper sign for credit)

What is the enthalpy change of this reaction. Type the number and include a sign. DO NOT INCLUDE UNITS

Use the bond energy data below to find the  ΔH  for 

2H₂O(g) ⟶  2H₂(g)  +  O₂(g)

•   +480 kJ

•   -480 kJ

•   -440 kJ

•   + 440 kJ

Tags

LM 54

_____ Hydrogen-Hydrogen single bond/s are broken and _____ Carbon-Hydrogen single bond/s formed

• 6; 8

• 2; 8

• 2; 10

• 6; 10

Breaking bonds is _________________. Forming bonds is ______________________

• endothermic, exothermic

• exothermic, endothermic

Using bond energies to solve for enthalpy, which formula would be correct?

• ΔH =  Bond broken - bonds formed

• ΔH =  Bond formed- bonds broken

• ΔH =  products - reactants

• ΔH =  reactants- products

Th average bond enthalpies are as follows:
H-H = 436 kJ/mol
Cl-Cl = 242 kJ/mol
H-Cl = 431 kJ/mol

What is the enthalpy change for the decomposition of hydrogen chloride?
2 HCl --> H₂ + Cl₂

• -184 kJ
• + 184 kJ
• - 247 kJ
• + 247 kJ

Shown above are the equation representing the decomposition of H2O2(l) and a table of bond enthalpies. On the basis of the information, which of the following is the enthalpy of decomposition of 2 mol of H2O2(l) ?

• −349kJ

• −203kJ

• 203kJ

• 349kJ