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250 mL of water is heated from 3 oC to 90 oC on a butane stove. Assume all the heat from combustion is used to warm the water. C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(l) Standard Enthalpies of Formation (ΔHof): C4H10(g) = -124.8 kJ /mol CO2(g) = -393.5 kJ /mol H2O(l) = -285.8 kJ /mol a) What is the total amount of heat required for the process? b) What is the molar heat of combustion for butane? c) What is the mass of butane needed for this process? (Please note that you must include units throughout all of your calculations and provide your answer in scientific notation to the correct number of significant digits.)
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