Consider the combustion of natural gas. also called methane (CH_a). Using the th

Question

Consider the combustion of natural gas. also called methane (CH_a). Using the thermodynamic data provided. answer the questions below. Be sure to use units in your work and final answers. Calculate DM_^and DS_^Is this reaction always, never, or sometimes spontaneous? Do you expect it to be "more spontaneous" at lower or higher temperature? Calculate DG_^for the combustion of methane at room temperature (a) and at the temperature that paper bums (b). (a) T = 22 degree C (b) T = 233 degree C From this calculation, which of these reactions has a larger driving force to occur (which is "more spontaneous"). Is this what you expected? Give some discussion of why you expected this or why this may be surprising.

Explanation / Answer

Q6.

dH = Hproducts - Hreactants

dH = H-CO2 + 2*H-H2O - (H-CH4 + 3*H-O2)

dH = -393.5 + 2*-241.8 - (-74.8 + 3*0) = -802.3 kJ/mol

For

dS:

dS = Sproducts - Sreactants

dS = S-CO2 + 2*S-H2O - (S-CH4 + 3*S-O2)

dS = 213.7+ 2*188.72- (186.2+ 3*205) = -210.06 J/molK

Q7.

We need dG:

dG = dH - T*dS

dG = -802.3 *1000 - 298 * (-210.06 ) = -739702.12 J/mol = -739.70 k/mol

This is spontanous at low T

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