Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g)

Question

          Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the following reaction
2SO2+O2=2SO3
          The standard enthalpies of formation for SO2(g) and SO3(g) are
deltaH= SO2(g)= -296.8 kj
dH= SO3(g)=        -395.7 kJ

          Calculate the amount of energy in the form of heat that is produced when a volume of 3.75 L of SO2(g) is converted to 3.75 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0           Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the following reaction
2SO2+O2=2SO3
          The standard enthalpies of formation for SO2(g) and SO3(g) are
deltaH= SO2(g)= -296.8 kj
dH= SO3(g)=        -395.7 kJ

          Calculate the amount of energy in the form of heat that is produced when a volume of 3.75 L of SO2(g) is converted to 3.75 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0      Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the following reaction
2SO2+O2=2SO3
          The standard enthalpies of formation for SO2(g) and SO3(g) are
deltaH= SO2(g)= -296.8 kj
dH= SO3(g)=        -395.7 kJ

          Calculate the amount of energy in the form of heat that is produced when a volume of 3.75 L of SO2(g) is converted to 3.75 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0 Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the following reaction
2SO2+O2=2SO3
          The standard enthalpies of formation for SO2(g) and SO3(g) are
deltaH= SO2(g)= -296.8 kj
dH= SO3(g)=        -395.7 kJ

          Calculate the amount of energy in the form of heat that is produced when a volume of 3.75 L of SO2(g) is converted to 3.75 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0           The standard enthalpies of formation for SO2(g) and SO3(g) are
deltaH= SO2(g)= -296.8 kj
dH= SO3(g)=        -395.7 kJ
     The standard enthalpies of formation for SO2(g) and SO3(g) are
deltaH= SO2(g)= -296.8 kj
dH= SO3(g)=        -395.7 kJ
The standard enthalpies of formation for SO2(g) and SO3(g) are
deltaH= SO2(g)= -296.8 kj
dH= SO3(g)=        -395.7 kJ
          Calculate the amount of energy in the form of heat that is produced when a volume of 3.75 L of SO2(g) is converted to 3.75 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0      Calculate the amount of energy in the form of heat that is produced when a volume of 3.75 L of SO2(g) is converted to 3.75 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0 Calculate the amount of energy in the form of heat that is produced when a volume of 3.75 L of SO2(g) is converted to 3.75 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0

Explanation / Answer

using the idela gas equation,

PV=nRT

or 1*3.75=n*(298/12)

or n=0.15 moles

enthalpy of the reaction=-395.7 + 296.8

= -98.9 kJ/mol

so energy produced=0.15*98.9

=14.835 kJ

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