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Part A The combustion of methane gas, the principal constituent natural gas, is represented by the equation CH, (g) + 20 (9) + CO2(g) + 2 H20 (1) AH = -890.3 kJ mol-1 You may want to reference (Page) Section 7.1 while completing this problem. What mass of methane, in kilograms, must be burned to liberate 3.20x107 kJ of heat? Express your answer to three significant figures. th + IVO A ? 1 = kg Submit Request Answer Part B What quantity of heat, in kilojoules, is liberated in the complete combustion of 1.50x10' L of CH4(9), measured at 18.8°C and 766 mmHg Express your answer to three significant figures. VOI Ad th + ? k.) Submit Request Answer Part 6 If the quantity of heat calculated in part B could be transferred with 100% elficiency to water, what volume of water, in liters, could be heated from 9.4 to 60.0 °C as a result? Express your answer to three significant figures. ΤΡΗ ΑΣΦ ? Pearson