Sulfur trioxide, SO3, can be removed from the exhaust gases of power plants by reaction with lime, CaO, according the the equation, Cao(s) + SO3(g) → CaSO4(s) AH-976.91 kJ If 2.04 kg of SO3 is to be removed, how much heat (in megajoules) is released? Atomic masses: 0 = 16 g/mol Ca = 40 g/mol S = 32 g/mol (Round answer to the second decimal place.)

Sulfur trioxide, SO3, can be removed from the exhaust gases of power plants by reaction with lime, CaO, according the the equation, Cao(s) + SO3(g) → CaSO4(s) AH-976.91 kJ If 2.04 kg of SO3 is to be removed, how much heat (in megajoules) is released? Atomic masses: 0 = 16 g/mol Ca = 40 g/mol S = 32 g/mol (Round answer to the second decimal place.)

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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Determine the amount of heat released when 180.00 g AsBr5(g) reacts according to the following equation: As4O10(g) + 6 AsBr5(g) → 10 Br3AsO(g) Additional equations that may be useful: 1/4 As4(s) + 3/2 Br2(g) → AsBr3(g) ΔH = -336.4 kJ/mol As4(s) + 5 O2(g) → As4O10(g) ΔH = -2967.3 kJ/mol AsBr3(g) + Br2(g) → AsBr5(g) ΔH = -84.2 kJ/mol AsBr3(g) + 1/2 O2(g) → Br3AsO(g) ΔH = -295.7 kJ/mol
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