Compute net heat of combustion for 3.5 moles isobutane(C_6H_10). Standard of for
ID: 1068657 • Letter: C
Question
Compute net heat of combustion for 3.5 moles isobutane(C_6H_10). Standard of formula for C_4 H_10 isobutane is 131.6 kJ/mol -7954.2 kJ -10605.6 kJ -6628.5kj -9279.9 kj -5302.8 kj Compute gross heat of combustor for 4.5 moles of isobutane (C_4H_10). Standard enthalpy of formation for C_4H_10 isobutane is -131.6 KJ/mol -11485 6 KJ -8614.2 Kj -7178.5 KJ -12921.3 KJ -5742.8 KJ Consider three monitoring wells each located at the vertex of an equilibrium triangle. The distance between any pair of wells is a 3000 m. The head in each well reference to some common datum, are as follows well 1.950m. well 2, 100.3 m. well 3 100.3 m. Find the magnitude of the hydraulic gradient 0.03964 0.00115 0.0204 0.00099 0.00087 Express 50.0 ppmv of Nitric Oxide (NO) in mg/m^3 at 25 C 122.62 mg/m^3 61.31 mg/m^3 110.36 mg/m^3 12.26 mg/m^3 49.05 mg/m^3Explanation / Answer
Heat of Combustion of Isobutane 361 Utilizing the values for the heats of formation of carbon dioxide and of water given in an earlier paper [3], the following values are obtained for the heat of formation of isobutane at 25° C: 4 C (c, (3 graphite)+5 H2 (gas)=iso-C4H10 (gas), LlH0298.1 = -32.20 ± 0.43 kilocalories pel' mole; 4 C (c, diamond) +5 H2 (gas)=iso-C4H10 (gas), LlH0298.1 = -33.08 ± 0.43 kilocalories per mole. Combination of the pre3ent value for the heat of combustion of isobutane with that previously reported for normal butane will yield a reliable value for the difference in the energies of formation of the two isomers. With no significant impurity in the reaction (see page 358), the reliability of the relatively small difference in the two values of the heats of combustion will be determined by the precision of the two values rather than by the absolute accuracy. The precision uncertainties of the calorimetric combustion experi-ments are, respectively, ± 0.018 and ± 0.013 percent, or ± 0.52 and ± 0.37 kilojoule per mole, for normal butane and isobutane. Taking the uncertainty in the difference in the two heats of combustion as the square root of the sum of the squares of the foregoing quantities, one obtains for the following reaction, at 25° C and 1 atmosphere, n-C4H10 (gas)=iso-C4H10 (gas), Ml298.1 = -6.82 ± 0.64 kilojoules, or -1.63 ± 0.15 kilocalories, per mole. Since for the two isomers, at room temperature and a pressure of 1 atmosphere, the values of PV, and of E (P=l)-E (P=O), are not significantly different, one can write for the above reaction LlH0298.1 =LlE0298.1=-1.63 ± 0.15 kilocalories pel' mole. This value indi-cates that at 25° C the internal or intrinsic energy of isobutane is less than that of normal butane by 1.63 ± 0.15 kilocalories per mole. There is extant in the literature no value with which this can be compared.3 This new value for the heat of combustion of isobutane has also been utilized in conjunction with the previously reported data [2, 3] on methane, ethane, and propane, to deduce a fairly reliable value for the heat of combustion and of formation of tetramethylmethane (neopentane) [8].
answer 37) d
38) c
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