Sulfur (2.55 g) was burned in a constant volume calorimeter with excess O₂(g). The temperature increased from 20.56 °C to 25.78 °C. The bomb has a heat capacity of 933 J/K, and the calorimeter contained 858 g of water. (Specific heat capacity of water is 4.184 J/g. K.) Calculate AU per mole of SO2 formed for the reaction. S8 (s) + 8 O₂ (g) → 8 SO₂ (g) Sulfur burns in oxygen with a bright blue flame to give SO₂ (g). AU = kJ/mol SO₂

Sulfur (2.55 g) was burned in a constant volume calorimeter with excess O₂(g). The temperature increased from 20.56 °C to 25.78 °C. The bomb has a heat capacity of 933 J/K, and the calorimeter contained 858 g of water. (Specific heat capacity of water is 4.184 J/g. K.) Calculate AU per mole of SO2 formed for the reaction. S8 (s) + 8 O₂ (g) → 8 SO₂ (g) Sulfur burns in oxygen with a bright blue flame to give SO₂ (g). AU = kJ/mol SO₂

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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