Did I Convert 5 Pounds of Nitroglycerin to Moles Correctly?

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SUMMARY

The discussion centers on converting 5 pounds of nitroglycerin into moles for a chemistry problem involving gas volume produced from its decomposition. The user correctly multiplied 5 pounds by 453 grams to convert to grams and then divided by the molar mass of nitroglycerin to find the number of moles. The primary concern raised is the appropriate temperature and pressure to use in the ideal gas law equation PV=nRT, with the consensus suggesting standard temperature and pressure (STP) as the default condition.

PREREQUISITES
  • Understanding of stoichiometry and chemical equations
  • Familiarity with the ideal gas law (PV=nRT)
  • Knowledge of molar mass calculations
  • Basic concepts of standard temperature and pressure (STP)
NEXT STEPS
  • Research the molar mass of nitroglycerin (C3H5N3O9)
  • Learn about the implications of using different temperatures and pressures in gas calculations
  • Explore stoichiometric calculations for gas reactions
  • Study the principles of gas laws and their applications in chemistry
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ngu9997
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Homework Statement


5 lbs of nitroglycerin detonates. What is the total volume of the gases produced?

Homework Equations


PV=nRT

The Attempt at a Solution


I used the balance chemical equation of the decomposition of nitroglycerin and used stoichiometry to find the number of moles of nitrogen, oxygen, and carbon dioxide added them all and put the number of moles into PV=nRT. The only thing I'm unsure about is how to convert 5 pounds of nitroglycerin into moles. I multiplied 5 pounds by 453 grams then divided by nitroglycerin's molar mass. Did i convert to moles correctly?
 
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ngu9997 said:
I multiplied 5 pounds by 453 grams then divided by nitroglycerin's molar mass. Did i convert to moles correctly?

Yes.
 
The real question is what temperature and pressure are you supposed to use?
 
When nothing else is given, I would assume STP.
 

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