Sulfur (2.34 g) was burned in a constant volume calorimeter with excess O₂ (g). The temperature increased from 20.35 °C to 26.27 °C. The bomb has a heat capacity of 922 J/K, and the calorimeter contained 654 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

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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.157QP: Consider the Haber process: N2(g)+3H2(g)2NH3(g);H=91.8kJ The density of ammonia at 25C and 1.00 atm...
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Sulfur (2.34 g) was burned in a constant volume calorimeter
with excess O₂ (g). The temperature increased from 20.35 °C
to 26.27 °C. The bomb has a heat capacity of 922 J/K, and the
calorimeter contained 654 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
Transcribed Image Text:Sulfur (2.34 g) was burned in a constant volume calorimeter with excess O₂ (g). The temperature increased from 20.35 °C to 26.27 °C. The bomb has a heat capacity of 922 J/K, and the calorimeter contained 654 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
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