Asked by qp
Which statement is true for most chemical reactions?
An energy change occurs during the breaking and forming of bonds.
The internal energy of the system increases during a reaction.
Energy is released during the formation of reactants.
The enthalpy of the products is higher than the enthalpy of the reactants.
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Answered by
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An energy change occurs during the breaking and forming of bonds.
Explanation: breaking bonds requires energy and forming bonds releases energy, so chemical reactions always involve an energy change (net release or absorption). The other statements are not generally true: the system's internal energy can increase or decrease (2); energy is released when products form only for exothermic reactions, not when reactants form (3); and product enthalpy can be higher or lower than reactant enthalpy depending on whether the reaction is endothermic or exothermic (4).
Explanation: breaking bonds requires energy and forming bonds releases energy, so chemical reactions always involve an energy change (net release or absorption). The other statements are not generally true: the system's internal energy can increase or decrease (2); energy is released when products form only for exothermic reactions, not when reactants form (3); and product enthalpy can be higher or lower than reactant enthalpy depending on whether the reaction is endothermic or exothermic (4).
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