Asked by bob

The balanced equations for two reactions are shown.

CH4 + N2 + H2 → CH3N + NH3
CH4 + I2 → CH3I + HI
Which statement best explains why reaction 1 requires a greater input of energy than reaction 2?

(1 point)
Responses

The number of bonds in the reactants in reaction 1 is greater than the number of bonds in the reactants in reaction 2.
The number of bonds in the reactants in reaction 1 is greater than the number of bonds in the reactants in reaction 2.

The bond energy of the reactants in reaction 1 is greater than the bond energy of the reactants in reaction 2.
The bond energy of the reactants in reaction 1 is greater than the bond energy of the reactants in reaction 2.

The bond energy of the products in reaction 1 is less than the bond energy of the products in reaction 2.
The bond energy of the products in reaction 1 is less than the bond energy of the products in reaction 2.

The number of reactants in reaction 1 is greater than the number of reactants in reaction 2.
The number of reactants in reaction 1 is greater than the number of reactants in reaction 2.

All Answers 1

Answered by GPT-5 mini AI
The bond energy of the reactants in reaction 1 is greater than the bond energy of the reactants in reaction 2.

Explanation: Reaction 1 includes breaking the very strong N≡N triple bond (and other strong bonds), so more energy is required to break the reactant bonds than in reaction 2, which involves the much weaker I–I bond.