Calculate the energy required to break the bonds in propane (C3H8) given the following bond energies: C-C = 347 kJ/mol; C-H = 413 kJ/mol.

To calculate the energy required to break the bonds in propane (C3H8), we need to consider the number and type of bonds in a molecule of propane.

Propane has three C-C bonds and eight C-H bonds.

Step 1: Calculate the energy required to break the C-C bonds. There are 3 C-C bonds in propane, and the energy required to break one C-C bond is 347 kJ/mol. So, the total energy required to break all the C-C bonds is 3 * 347 kJ/mol = 1041 kJ/mol.

Step 2: Calculate the energy required to break the C-H bonds. There are 8 C-H bonds in propane, and the energy required to break one C-H bond is 413 kJ/mol. So, the total energy required to break all the C-H bonds is 8 * 413 kJ/mol = 3304 kJ/mol.

Step 3: Add the energy required to break the C-C bonds and the C-H bonds. The total energy required to break all the bonds in propane is 1041 kJ/mol (from the C-C bonds) + 3304 kJ/mol (from the C-H bonds) = 4345 kJ/mol.

So, the energy required to break the bonds in propane (C3H8) is 4345 kJ/mol.