I need help with chemistry heat

Question

Methane is the principal component of natural gas, and probably the most abundant organic compound on earth. Its abundance makes it an attractive option for fuel, however, it is a potent greenhouse gas.

CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) ΔH = -890 kJ/mol ΔS = -242 J/K

(a) On your own sheet of paper, sketch the energy diagram that would result for this reaction. Label the activation energy (Ea) and the enthalpy change (ΔH) in your diagram.

(b) Replace each chemical formula in the equation above with a Lewis structure for each molecule.  

(c) A table of bond enthalpies if provided below. Calculate the bond enthalpy for the carbon-to-oxygen bond present in carbon dioxide.

Covalent bond	Bond enthalpy (kJ/mol)
C - H	413
O = O	495
O - H	463

(d) Based on the enthalpy and entropy of this reaction, would you expect the combustion of methane to always occur spontaneously, never occur spontaneously, or would it be temperature dependent? Justify your choice with a complete explanation.

Answer 1

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