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Find the standard enthalpy of formation of ethylene, C2H4(g), given the following...
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The heat of reaction of a particular chemical reaction can be expressed as:
`H_(reaction) = sum[n Delta H^0_(f) p r oducts] -sum[n Delta H^0_(f) react a nts ] `
Where n = number of moles in the balanced chemical equation
Sum of heat of formation of the products `= [2 mol CO_2* -393.5 (kJ)/(mol)] + [2 mol H_(2)O * -285.8 (kJ)/(mol)] =-1358.6 kJ`
Sum of heat of formation of reactants `= Delta H^0_(f) _(ethyl e n e) + 0`
note: Oxygen has a `Delta H^(0)_(f)` of 0
Substituting these values to the first equation:
`-1411 kJ = -1358.6 kJ - Delta H^0_(f) _(ethyl en e) `
`Delta H^0_(f) _(ethyl en e) = -1358.6 kJ - (-1411kJ) `
`Delta H^0_(f) _(ethyl en e) = + 52.4 kJ -> answer`
Posted by jerichorayel on October 27, 2013 at 2:37 AM (Answer #1)
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