Question

calculate the heat of reaction \\( \delta h \\) for the following reaction:

\\( 2 \mathrm { ch } _ { 4 } ( g ) + 3 \mathrm { o } _ { 2 } ( g ) \
ightarrow 2 \mathrm { co } ( g ) + 4 \mathrm { h } _ { 2 } \mathrm { o } ( g ) \\)

you can find a table of bond energies by using the data button on the aleks toolbar.

round your answer to the nearest \\( \mathrm { kj } / \mathrm { mol } \\).

Explanation:

Step1: List bond energies (typical values)

C-H: 413 kJ/mol; O=O: 498 kJ/mol; C≡O: 1072 kJ/mol; O-H: 464 kJ/mol

Step2: Calculate bonds broken (reactants)

2 CH₄: 2×4×C-H = 8×413 = 3304 kJ/mol
3 O₂: 3×O=O = 3×498 = 1494 kJ/mol
Total broken: 3304 + 1494 = 4798 kJ/mol

Step3: Calculate bonds formed (products)

2 CO: 2×C≡O = 2×1072 = 2144 kJ/mol
4 H₂O: 4×2×O-H = 8×464 = 3712 kJ/mol
Total formed: 2144 + 3712 = 5856 kJ/mol

Step4: Compute ΔH

ΔH = bonds broken - bonds formed = 4798 - 5856 = -1058 kJ/mol

Answer:

-1058 $\frac{\text{kJ}}{\text{mol}}$