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TX PACT Chemistry Grades 7-12 Sample Test

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The following energies are held in different types of bonds:

C – H bond: 415kJ.

Cl –Cl bond: 243kJ.

C – Cl bond: 330kJ.

H – Cl bond: 432 kJ.

What is the net energy change associated with the following reaction given this information?

                                    CH4(g) + 2 Cl2 (g) --> CH2Cl2 (g) + 2 HCl (g)





Correct Answer:
-208kj.
to determine the net energy change for the given chemical reaction, we first need to understand the concept of bond enthalpies and how they affect the energetics of a reaction. bond enthalpies (or bond dissociation energies) represent the energy required to break one mole of a bond in a molecule in the gas phase, usually expressed in kilojoules per mole (kj/mol).

the reaction we are considering is: \[ \text{ch}_4(g) + 2\text{cl}_2(g) \to \text{ch}_2\text{cl}_2(g) + 2\text{hcl}(g) \] in this reaction: - **breaking bonds**: bonds are broken in the reactants, which requires energy. - **forming bonds**: bonds are formed in the products, which releases energy.

let’s calculate the total energy changes involving breaking and forming of bonds: - **bonds broken**: - two c–h bonds in ch4 (2 x 415 kj = 830 kj) - two cl–cl bonds in cl2 (2 x 243 kj = 486 kj) total energy required to break bonds = 830 kj + 486 kj = 1316 kj - **bonds formed**: - two c–cl bonds in ch2cl2 (2 x 330 kj = 660 kj) - two h–cl bonds in hcl (2 x 432 kj = 864 kj) total energy released in forming bonds = 660 kj + 864 kj = 1524 kj

to find the net energy change of the reaction, we subtract the total energy used to break bonds from the total energy released by forming bonds: \[ \text{net energy change} = \text{energy released} - \text{energy required} \] \[ \text{net energy change} = 1524 \text{ kj} - 1316 \text{ kj} \] \[ \text{net energy change} = 208 \text{ kj} \] therefore, the net energy change for the reaction is -208 kj, indicating that the reaction is exothermic. this means that more energy is released in forming the products than is required to break the bonds in the reactants, leading to a release of energy to the surroundings.


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