Look at the equation showing the splitting of water to give hydrogen and oxygen . Use it to find the energy released by forming bonds in this reaction. You will need some of the bond energies from the table. Enter your answer as a number kJ/mol 2H_(2)Oarrow 2H_(2)+O_(2) Bond Bond energy (kJ/mol) Harrow H 436 O=O 498 H-O 464 C-H 413 C=0 803 Nequiv N 945 N+A 391 243 H-Cl 432

## Step 1: Identify Bonds Broken in Reactants### In the reaction , each water molecule ( ) has two bonds. Therefore, for 2 molecules, a total of 4 bonds are broken.## Step 2: Calculate Energy Required to Break Bonds### The bond energy for is 464 kJ/mol. Thus, the total energy required to break 4 bonds is kJ.## Step 3: Identify Bonds Formed in Products### In the products, 2 molecules are formed, each with one bond, and 1 molecule is formed with one bond. Therefore, 2 bonds and 1 bond are formed.## Step 4: Calculate Energy Released by Forming Bonds### The bond energy for is 436 kJ/mol, and for is 498 kJ/mol. Thus, the total energy released by forming 2 bonds and 1 bond is \((2 \times 436) + 498 = 872 + 498 = 1370\) kJ.## Step 5: Determine Net Energy Change### The net energy change is the difference between the energy required to break the bonds and the energy released by forming the bonds: kJ.#