Thermochemistry

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[Eem05]

C6H12O6 + 6O2 ---> 6CO2 + 6H2O
Heat of Reaction: -2803kJ/mol

At the top of Mt. Everest--
1. How many moles of reaction must occur per minute to satisfy a mountain climber's energy requirement of 34.867kJ/min?
2. How many grams of O2 must be consumed per minute to satisfy the climber's need?
3. How many liters/min of air must the mountain climber breathe (assuming 100% efficiency in each breath of extracting O2 out of the air)?

1. Would using the energy requirement and the determined heat of reaction in an equation to cancel the appropriate units give me the number of moles/minute?
2. I understand that there are -467.16kJ/mol of O2.  Do I convert this with the energy requirement to get moles of O2 and then convert that to grams of O2 using the Molar Mass?
3. I think I use the density of O2 here but am slightly confused still.

Any push in the right direction or hints of any kind would be greatly appreciated.  I just feel overwhelmed with information and don't know where to start. Thanks!

[mr_cochran]

Well, good start,
1) You can determined the moles of glucose per minute as you've stated.
2) From the above you should be able to determine the moles oxygen required and thus mass of oxygen.
3) Density of a gas varies with temperature and pressure; are these quantities revealed in this or previous problems? If not then assume STP, not a good assumption at the top of Mt Everest though.