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Category > Chemistry Posted 19 Jun 2017 My Price 6.00

Standard Enthalpies of Formation (ΔHof)

  1. 250 mL of water is heated from 3 oC to 90 oC on a butane stove. Assume all the heat from combustion is used to warm the water.

C4H10(g) + 13/2 O2(g) → 4 CO2(g) + 5 H2O(l)

Standard Enthalpies of Formation (ΔHof):

 

  • C4H10(g) = -124.8 kJ/mol
  • CO2(g) = -393.5 kJ/mol
  • H2O(l) = -285.8 kJ/mol
  1. What is the total amount of heat required for the process?
  2. What is the molar heat of combustion for butane?
  3. What is the mass of butane needed for this process?

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SuperTutor
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Status NEW Posted 19 Jun 2017 03:06 AM My Price 6.00

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