200. g of liquid phase octane (C8H18) are burned in air at a temperature of 100....

200. g of liquid phase octane (C8H18) are burned in air at a temperature of 100. degrees Celsius and a pressure of 1.00 atm, forming vapor phase water and carbon dioxide.

a) Write the balanced chemical reaction equation for this process.

b) What is the magnitude of the difference between ΔE and ΔH for one mole of octane going through this process? (Hint: use the value of R that makes life easiest.)

c) The reaction is in contact with a reservoir of water that is also at 100 degrees Celsius. If that reservoir absorbs all of the heat released by the reaction (of the 200. g of octane), how many moles of the water will evaporate? Each mole of C8H18 releases 5074.482 kJ of heat when it goes through this process.

Part a I got no problem, but I can't seem to figure out parts b and c. Thanks for the help!!

Expert Solution

queen_honey_blossom answered 2 years ago

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