Bond Energy

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

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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)

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NGSS.HS-PS1-4

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NGSS.HS-PS1-4

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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

• 2045 kJ endothermic

• -2045 kJ exothermic

• 2045 kJ exothermic

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NGSS.HS-PS1-4

NGSS.HS-PS3-1

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NGSS.HS-PS1-4

NGSS.HS-PS3-1

Use bond energies to determine the energy change for the following reaction and use the information to determine if it is an endothermic or exothermic reaction: HCN + H₂ --> CH₃N₂

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NGSS.HS-PS1-4

Which of the following bonds has the highest bond energy?

• C-H bond

• O=O bond

• N≡N bond

• C=C bond

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NGSS.HS-PS1-4

Bond energy is defined as the amount of energy required to:

• Break one mole of bonds in gaseous molecules

• Form one mole of bonds in gaseous molecules

• Break one mole of bonds in liquid molecules

• Form one mole of bonds in liquid molecules

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NGSS.HS-PS1-4

In a chemical reaction, if the bond energies of the reactants are higher than the bond energies of the products, the reaction is:

• Endothermic

• Exothermic

• Isothermal

• Adiabatic

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NGSS.HS-PS1-4