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RICKYandCINDY
RICKYandCINDY asked in Science & MathematicsChemistry · 5 years ago

the standard heat of formation of glucose is -1260 kJ/mol calculate how much heat is released at standard conditions if 1 mol undergoes this?

Update:

The standard heat of formation of glucose is -1260 kJ/mol calculate how much heat is released at standard conditions if 1 mol undergoes this reaction?

C6H12O6 (s) + 6O2(g) ---> 6CO2 (g) + 6H2O

Update 2:

how would one do this?

Thanks

Update 3:

Is it 1260 kJ?

2 Answers

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  • Anonymous
    4 years ago

    Heat Of Formation Of Glucose

    Source(s): https://owly.im/a8P0r
  • ?
    Lv 7
    5 years ago

    This is a Hess's law problem

    the heat of formation reaction for glucose is

    6C(s, graphite) + 6H2(g) + 3O2(g) ---> C6H12O6(s) .... delta H = -1260 kJ / mole of glucose

    note the states !!

    we also need the delta Hf for CO2 and H2O

    CO2 (g) -393.5 kJ / mol

    H2O (l) -285.8 kJ / mol

    so for the equation

    C6H12O6 (s) + 6 O2 (g) ---> 6 CO2 (g) + 6 H2O (l)

    we have

    ΔH°rxn = Σ ΔH°f (products) minus Σ ΔH°f (reactants)

    ΔH°rxn = [ 6 (-393.5) + 6 (-285.8) ] minus [ (-1275) + (6) (0) ]

    = -2801 kJ/mol of glucose.

    excellent solution ?? best answer please ?

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