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23 Nov 2019

A 12-gram mixture of methane, CH4, and ethane, C2H6, is completelycombusted in oxygen. If the total mass of H2O produced is 23.4grams, what was the approximate mass of the methane in the originalmixture?

A. 4 g CH4
B. 8 g CH4
C. 5 g CH4
D. 6 g CH4

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Casey Durgan
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19 Feb 2019

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Related questions

An important reaction for the conversion of natural gas to other useful hydrocarbons is the conversion of methane to ethane.

2 CH4(g) C2H6(g) + H2(g)

In practice, this reaction is carried out in the presence of oxygen, which converts the hydrogen produced into water.

2 CH4(g) + O2(g) C2H6(g) + H2O(g)

Use Table 8.4 to estimate ∆H for these two reactions. Why is the conversion of methane to ethane more favorable when oxygen is used?

A mixture of methane (CH4) and propane (C3H8) has a total mass of 29.84 g. When the mixture is burned completely in excess oxygen, the CO2 and H2O products have a combined mass of 142.97 g. What is the mass of methane in the original mixture?

The conversion of natural gas, which is mostly methane, into products that contain two or more carbon atoms, such as ethane (C2H6), is a very important industrial chemical process. In principle, methane can be converted into ethane and hydrogen:

2 CH4(g) C2H6(g) + H2(g)

In practice, this reaction is carried out in the presence of oxygen:

2 CH4(g) + O2(g) C2H6(g) + H2O(g)

(a) Using the data in Appendix C, calculate K for these reactions at 25 °C and 500 °C. (b) Is the difference in ∆G° for the two reactions due primarily to the enthalpy term (∆H) or the entropy term (-T∆S)? (c) Explain how the preceding reactions are an example of driving a nonspontaneous reaction, as discussed in the “Chemistry and Life” box in Section 19.7. (d) The reaction of CH4 and O2 to form C2H6 and H2O must be carried out carefully to avoid a competing reaction. What is the most likely competing reaction?

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