Bond enthalpy practice problems

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

Tags

NGSS.HS-PS1-4

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

Tags

NGSS.HS-PS1-4

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)

Tags

NGSS.HS-PS1-4

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

Tags

NGSS.HS-PS1-4

100 kJ of energy is introduced to your cell phone while it charges but 10 kJ of energy is lost as work in the process as heat given off to the surroundings. What is ΔE for the system? You have ΔE = q + w

•   +90 kJ

•   +110 kJ

•   -90 kJ

•   -110 kJ

Tags

NGSS.HS-PS3-1

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

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

Tags

NGSS.HS-PS1-4

An equation representing the dissociation of O₂(g) into two oxygen atoms, and a table of bond enthalpies are shown above. Based on the information, which of the following is the enthalpy of dissociation for O₂(g)?

• −641kJ/mol

• −495kJ/mol

• 495kJ/mol

• 641kJ/mol

Tags

NGSS.HS-PS1-4

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

• 6; 8

• 2; 8

• 2; 10

• 6; 10

Tags

NGSS.HS-PS1-7

_____ Carbon-Carbon single bond/s are formed

• 6

• 2

• 3

• 10