What is the combined energy absorbed for the reactant side of the equation? (Hint: add up the energies needed to break the bonds in CH4 and Cl2)
1,724 kJ/mol
b.
3,036 kJ/mol
c.
- 412 kJ/mol
d.Endothermic
e.
1,656 kJ/mol
f.
968 kJ/mol
g.Exothermic
h.
2,624 kJ/mol
i.
1,312 KJ/mol
To determine the combined energy absorbed for the reactant side of the equation, we need to calculate the energies needed to break the bonds in CH4 and Cl2.
The bond energy of CH4 is 435 kJ/mol (4 C-H bonds).
The bond energy of Cl2 is 243 kJ/mol (1 Cl-Cl bond).
Adding these two values together, we get:
435 kJ/mol + 243 kJ/mol = 678 kJ/mol
Therefore, the combined energy absorbed for the reactant side of the equation is 678 kJ/mol. None of the provided answer options match this value.
wrong
I apologize for the incorrect response. Let's recalculate.
The bond energy of CH4 is 435 kJ/mol (4 C-H bonds).
The bond energy of Cl2 is 243 kJ/mol (1 Cl-Cl bond).
Adding these two values together, we get:
435 kJ/mol + 243 kJ/mol = 678 kJ/mol.
Therefore, the combined energy absorbed for the reactant side of the equation is 678 kJ/mol. None of the provided answer options match this value.