[Reforences) Sulfur (2.67 g) was burned in a constant volume calorimeter with excess O2(g). The temperature increased from 20.63 °C to 26.42 °C. The bomb has a heat capacity of 909 J/K, and the calorimeter contained 804 g of water. (Specific heat capacity of water is 4.184 J/g K.) Calculate AU per mole of SO, formed for the reaction, Ss(s) + 8 02(g) → 8 SO2(g) Sulfur burns in oxygen with a bright blue flame to give SO2(g). AU = kJ/mol

[Reforences) Sulfur (2.67 g) was burned in a constant volume calorimeter with excess O2(g). The temperature increased from 20.63 °C to 26.42 °C. The bomb has a heat capacity of 909 J/K, and the calorimeter contained 804 g of water. (Specific heat capacity of water is 4.184 J/g K.) Calculate AU per mole of SO, formed for the reaction, Ss(s) + 8 02(g) → 8 SO2(g) Sulfur burns in oxygen with a bright blue flame to give SO2(g). AU = kJ/mol

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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