If the heat produced by the reaction of combustion of 1 mole of ethanol (MMethanol" 46.07 g/mol) is 1366.8 kJ/mol, (see the thermochemical equation below, formula of ethanol is C2H6O), how much heat in kJ is produced by the combustion of 155 g of ethanol at the same conditions? C2H6O(g) + 302(g) → 2CO2(g) + 3H2O(g); AH°rxn=-1366.8 kJ/mol O 8.818 O 2.11854 x10s O 4.06 x102 O 4.60x10 O 2.12x10$

If the heat produced by the reaction of combustion of 1 mole of ethanol (MMethanol" 46.07 g/mol) is 1366.8 kJ/mol, (see the thermochemical equation below, formula of ethanol is C2H6O), how much heat in kJ is produced by the combustion of 155 g of ethanol at the same conditions? C2H6O(g) + 302(g) → 2CO2(g) + 3H2O(g); AH°rxn=-1366.8 kJ/mol O 8.818 O 2.11854 x10s O 4.06 x102 O 4.60x10 O 2.12x10$

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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