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

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To calculate the volume of hydrogen needed to hydrogenate 50 grams of glycerol trioleate at 1 atm and 25 degrees Celsius, begin with the balanced reaction equation for hydrogenation. Determine the number of moles of glycerol trioleate, which is given as 0.057 moles. Use stoichiometry to find the moles of hydrogen required for complete hydrogenation. Apply the ideal gas law, PV = nRT, using the ideal gas constant of 0.082 to solve for the volume of hydrogen. This method will provide the necessary volume for the reaction under the specified conditions.
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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 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.
 
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Start with the reaction equation, this is simple stoichiometry.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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