ConstantSrenodic TableUnder certain nonstandard conditions, the oxidation of 1 molof SO2(g) to SO3(9) by O2(g) absorbs 89.4 kJ/mol ofheat.Part AThe heat of formation of SO3(g) is -204.1 kJ/mol underthese same conditions.Find the enthalpy of formation of SO2(g).SO2(g) + 02(g) → SO3(g)A,H = 89.4 kJ/molExpress your answer using one decimal place.AƒH = -293.5 kJ/molSubmitPrevious AnswersCompletedPart BDetermine the total heat absorbed by the reaction, in kJ, if 2.50 g of O2 is required to fully oxidize the SO, to SO3. The molar mass of O2 is 32.00 gmol-1kJ

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Under certain nonstandard conditions, the oxidation of 1 mol of SO2(g) to SO3(9) by O2 (g) absorbs 89.4 kJ/mol of heat. Part A The heat of formation of SO3(g) is -204.1 kJ/mol under these same conditions. Find the enthalpy of formation of SO2(g). SO-(9) + 02(9) → SO3(g) A,H = 89.4 kJ/mol Express your answer using one decimal place. A,H = -293.5 kJ/mol Submit Previous AnswerS Completed Part B Determine the total heat absorbed by the reaction, in kJ, if 2.50 g of O2 mol1. kJ

Under certain nonstandard conditions, the oxidation of 1 mol of SO2(g) to SO3(9) by O2 (g) absorbs 89.4 kJ/mol of heat. Part A The heat of formation of SO3(g) is -204.1 kJ/mol under these same conditions. Find the enthalpy of formation of SO2(g). SO-(9) + 02(9) → SO3(g) A,H = 89.4 kJ/mol Express your answer using one decimal place. A,H = -293.5 kJ/mol Submit Previous AnswerS Completed Part B Determine the total heat absorbed by the reaction, in kJ, if 2.50 g of O2 mol1. kJ

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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