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

[chemconfusion]

Homework Statement

Calculate the volume of H₂ required to completely hydrogenate 50 grams of glycerol trioleate at 1 atm pressure and 25 degrees Celcius. 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.

 

[Borek]

Start with the reaction equation, this is simple stoichiometry.

 

[Blueshift5]

I would approach this problem by first understanding the chemical reaction that is taking place. In this case, we are dealing with the hydrogenation of glycerol trioleate. This reaction involves the addition of hydrogen gas (H2) to the glycerol trioleate molecule, resulting in the formation of a saturated fat.

Next, I would gather all the necessary information, such as the given mass of glycerol trioleate (50 grams), the pressure (1 atm), and the temperature (25 degrees Celsius). I would also make sure to convert all units to the appropriate SI units (grams to moles, Celsius to Kelvin).

Then, I would use the ideal gas equation (PV = nRT) to calculate the number of moles of hydrogen gas needed for the reaction. The ideal gas constant (R) should also be converted to the appropriate units (0.082 L atm/mol K).

Once I have the number of moles of hydrogen gas, I can then use the molar mass of H2 (2 grams/mol) to calculate the mass of H2 needed. Finally, I can use the density of H2 at STP (standard temperature and pressure, 1 atm and 0 degrees Celsius) to convert the mass of H2 to volume.

In summary, the steps would be:

1. Understand the reaction and gather all necessary information.
2. Convert all units to SI units.
3. Use the ideal gas equation to calculate the number of moles of H2 needed.
4. Use the molar mass of H2 to calculate the mass of H2 needed.
5. Use the density of H2 at STP to convert the mass of H2 to volume.

I hope this helps guide you in solving the problem. Remember to always double-check your units and calculations to ensure accuracy. Good luck!