Calculating the vol. of hydrogen needed to hydrogenate under certain conditions

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SUMMARY

The discussion focuses on calculating the volume of hydrogen (H2) required to hydrogenate 50 grams of glycerol trioleate at 1 atm pressure and 25 degrees Celsius. The ideal gas constant used is 0.082, and it is established that 0.057 moles of glycerol trioleate need hydrogenation. Participants emphasize the importance of starting with the reaction equation and applying stoichiometry to derive the solution. The Ideal Gas Equation is confirmed as a necessary tool for this calculation.

PREREQUISITES
  • Understanding of stoichiometry in chemical reactions
  • Familiarity with the Ideal Gas Law and its applications
  • Knowledge of molar mass calculations for glycerol trioleate
  • Basic concepts of gas behavior under varying conditions
NEXT STEPS
  • Study the Ideal Gas Law and its application in chemical reactions
  • Learn how to calculate molar mass for organic compounds like glycerol trioleate
  • Explore stoichiometric calculations in hydrogenation reactions
  • Investigate the effects of temperature and pressure on gas volume
USEFUL FOR

Chemistry students, chemical engineers, and professionals involved in organic synthesis and hydrogenation processes will benefit from this discussion.

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Homework Statement

Calculate the volume of H2 required to completely hydrogenate 50 grams of glycerol trioleate at 1 atm pressure and 25 degrees celsius. The ideal gas constant is 0.082.



Homework Equations

I am unsure if I need the Ideal Gas Equation or not. I know that the ideal gas constant is 0.082 and that there are .057 moles of glycerol trioleate that need to be hydrogenized.



The Attempt at a Solution

I am at a loss at where to start. I am not necessarily looking for an answer, but guidance as to how to go about this.
 
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Start with the reaction equation, this is simple stoichiometry.
 

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