THE ANSWER IS ALSO NOT -15.79!!!!!!!! Sulfur dioxide, SO_2(g), can react with ox
ID: 1068324 • Letter: T
Question
THE ANSWER IS ALSO NOT -15.79!!!!!!!!
Sulfur dioxide, SO_2(g), can react with oxygen to produce sulfur trioxide, SO_3(g), by the following reaction 2SO_2 (g) + O_2(g) rightarrow 2SO_2(g) The standard enthalpies of formation for SO_2(g) and SO_3(g) are Delta H degree _f [SO_2 (g)] = -296.8 kJ/mol Delta H degree _f [SO_3 (g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 3.58 L of SO_2(g) is converted to 3.58 L of SO_3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0 degree C. Assume ideal gas behavior.Explanation / Answer
2SO2(g) + O2(g) ----> 2SO3(g))
DH0rxn = 2*DH0SO3 - (2*DH0SO2 + 1*DH0O2)
= (2*-395.7) - (2*-296.8+1*0)
= -197.8 kj
no of mole of SO2 = pv/RT = 1*3.58/(0.0821*298) = 0.146 mole
no of mole of SO3 = 1*3.58/(0.0821*298) = 0.146 mole
from above data ,
2 mole SO3 formation = -197.8 kj
0.146 mole SO3 formation = -197.8*0.146/2 = -14.44 kj
answer: amount of heat produced = 14.44 kj
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