1. Melted methane was ignited and used to heat water in a thin metal container. After a short period of time, themethane was extinguished and final measurements were made.Mass of methane before burningMass of methane after burningMass of water in containerInitial temperature of waterFinal temperature of water= 7.52 g= 7.20 g= 140.0 g= 10.0°C= 32.0°Ca) Using this data, calculate the heat of combustion of methane in kJ/mol. Assume that all the heat from themethane was absorbed by the waterb) Write the thermochemical equation for the complete combustion of methane. Selected Standard Molar Enthalpies of FormationAH₁AH;AH₁Substance (kJ/mol) Substance (kJ/mol) Substance (kJ/mol)Al₂O3(s)-1675.7 HBr(g)CaCO3(s)-1207,6 HCl(g)CaCl₂(s)Ca(OH)₂(s)CCL₂(E)CCL4(8)CHCI ()CH₂(g)C₂H₂(g)C₂H₁(g)C₂H₂(g)CzHs(g)CH()CH₂OH(E)C₂H₂OH()CO(g)CO₂(g)COCI₂(g)+49.1 Fe₂O₂(8)-239.2 Fe,O4(s)-277.6 FeCl₂(s)CH3COOH(E) –484.3 FeCls(s)-110.5 FeS (8)CS₂(e)CS₂(g)CrCla(g)Cu(NO₂)₂ (8)-795.4 HF(g)-985.2 HCN(g).-128.2 H₂O(E)-95.7 H₂O(g)CuO(s)CuCl(s)CuCl₂(s)-134.1 H₂O₂(e)-74.6 HNO (0)+227.4 H₂PO4(s)+52.4 H₂S(g)-84.0 H₂SO4(e)-103.8 FeO(s)–36.3|NH(8)-92.3 N₂H4(e)-273.3 NH Cl(s)+135.1 NH₂NO(s)-285.8 NO(g)-393.5 PbCl₂(s)-219.1 MgCl₂(s)+89.0 MgO(s)+116.7 Mg(OH)2(s)-556.5 HgS(s)-241.8 NO₂(g)-187.8 N₂O(g)-174.1 N₂O(g)1284.4 PH,(g)-20.6 PCl₂(g)814.0 P,O,(s)-272.0 P4O₁0(s)-824.2 KBr(s)-1118.4 KCl(s)-341.8 KCIO,(s)-399.5 KOH(s)-178.2 AgaCO₂ (s)-359.4 AgCl(s)-641.3 AgNO,(s)-601.6 Ag S(s)-924.5 SFB(g)-58.2 SO₂(g)-302.9 NaCl(s)-411.2 SO₂(g)-157.3 NaOH(s)-425.6 SnCl₂(s)-137.2 Na₂CO3(s)-1130.7 SnCl4(e)-220.1-45.9+50.6-314.4-365.6+91.3+33.2+81.6+11.1+5.4-287.0-2144.3-2984.0-393.8-436.5-397.7-424.6-505.8-127.0-124.4-32.6-1220.5-296.8-395.7-325.1-511.3Note: The enthalpy of formation of an element in its standard state isdefined as zero.

Enthalpy of combustion is defined as the amount of heat released by burning of one mole of compound.

1. Melted methane was ignited and used to heat water in a thin metal container. After a short period of time, the methane was extinguished and final measurements were made. Mass of methane before burning Mass of methane after burning Mass of water in container Initial temperature of water Final temperature of water = 7.52 g = 7.20 g = 140.0 g = 10.0°C = 32.0°C a) Using this data, calculate the heat of combustion of methane in kJ/mol. Assume that all the heat from the methane was absorbed by the water b) Write the thermochemical equation for the complete combustion of methane.

1. Melted methane was ignited and used to heat water in a thin metal container. After a short period of time, the methane was extinguished and final measurements were made. Mass of methane before burning Mass of methane after burning Mass of water in container Initial temperature of water Final temperature of water = 7.52 g = 7.20 g = 140.0 g = 10.0°C = 32.0°C a) Using this data, calculate the heat of combustion of methane in kJ/mol. Assume that all the heat from the methane was absorbed by the water b) Write the thermochemical equation for the complete combustion of methane.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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