General Chemistry 4th Edition this question has been customi

General Chemistry 4th Edition this question has been customized by Michael Ibele at Lindenwood University Mapu Sulfur dioxide, SO2(9), can react with oxygen to produce sulfur trioxide, SO3(g), by the following reaction 2502(g) +02(g) -> 2SO3(g) The standard enthalpies of formation for SO2(g) and SO3(g) are Hf |SC), (g) | =-296.8 kJ / mol 11,[SO3(g)]--395.7 kJ/mol Calculate the amount of energy in the form of heat that is given off when a volume of 2.70 L of So(g) is produced via this reaction at a constant pressure and temperature of 1.00 atm and 25.0 °C. Assume ideal gas behavior and that at the end of the reaction no left over reactants remain. Number kJ Next Exit Previous e Check Answer Hint

Solution

for the reaction, 2SO2(g)+ O2(g)<--------->2SO3(g)

standard heat of reaction = 2* standard heat of formation of SO3- {2* standard heat of formation of SO2+1*Standard heat of formation of O2}

where 2, 2 and 1 are coefficients of SO3, SO2 and O2 respectively.

since standard heat of formation of O2=0

standard enthalpy change of reaction = 2*(-395.7)- 2*(-296.8) =-197.8 Kj

one need to calculate the no of moles of SO3 generated during the course of reaction. This can be calculated from gas law equation, n= PV/RT

P= pressure in atm= 1, V= 2.7L, T= 25 deg.c= 25+273=298K, R= gas constant

n= PV/RT= 1*2.7/(0.0821*298)= 0.11 moles of SO3

2moles of SO3 gives off 197.8 KJ of energy ( since deltaH is -ve, there is heat generation)

0.11 moles of SO3 gvies 197.8*0.11/2 =10.9 Kj