General Chemistry 4th Edition University Science Books presented by Sapling Leam

Question

General Chemistry 4th Edition University Science Books presented by Sapling Leaming Maj Sulfur dioxide, SO2(9), can react with oxygen to produce sulfur trioxide, SO(g), by the following reaction The standard enthalpies of formation for SO2(g) and SO3(g) are AH SO,(2--2968 kJ/ mol H[sold] -395.7 kJ / mol Calculate the amount of energy in the form of heat that is produced when a volume of 3.34 L of SO(g) is converted to 3.34 L of SO:(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal gas behavior Number k.J Previous Give Up & View Solution Check Answer Next

Explanation / Answer

SO2 volume V = 3.34 L , P = 1bar = 0.987 atm , T = 25C = 25+273 = 298K

Using PV = nRT we will find moles of SO2 reacted or moles of SO3 formed ,  

0.987 atm x 3.34L = n x 0.08206Latm/molK x 298 K

n = 0.1348 mol = SO2 moles reacted = SO3 moles formed

dH reaction = 2 dH ( SO3) - 2 dH ( SO2) - dH ( O2)

= 2 ( -395.7) -2(- 296.8)

= - 197.8 KJ

per 2 moles dH = - 197.8 KJ , -ve sign indicates heat is produced ,

in our reaction we produced 0.1348 moles ,

hence heat = ( 197.8 KJ /2mol) x 0.1348 mol = 13.33

Thus heat produced = 13.33 KJ   

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