In the following reaction, the energy of the reactants is 1240 kJ/mol, and the bond energy of the products is 1790 kJ/mol. What is the total energy of the reaction? Is the reaction endothermic or exothermic?
A. 3030 kJ/mol, endothermic
B. -3030 kJ/mol, exothermic
C. 550 kJ/mol, endothermic
D. -550 kJ/mol, exothermic
The total energy of the reaction can be found by taking the difference between the energy of the reactants and the bond energy of the products:
Total energy = bond energy of products - energy of reactants
Total energy = 1790 kJ/mol - 1240 kJ/mol
Total energy = 550 kJ/mol
Since the total energy is positive, the reaction is endothermic. Therefore, the correct answer is C. 550 kJ/mol, endothermic.
To determine the total energy of the reaction, we need to find the difference between the energy of the reactants and the bond energy of the products.
Total energy of the reaction = Energy of reactants - Bond energy of products
Total energy of the reaction = 1240 kJ/mol - 1790 kJ/mol
Total energy of the reaction = -550 kJ/mol
Since the total energy of the reaction is negative (-550 kJ/mol), the reaction is exothermic.
Therefore, the correct answer is D. -550 kJ/mol, exothermic.