What is the Molecular Formula for a Compound Containing Nitrogen and Hydrogen?

[kevinf]

i have a question. the problem is

a compound contains only nitrogen and hydrogen and is 87.4% nitrogen by mass. a gaseous sample of the compound has a density of .977g/L at 710. torr and 100. degree celsius. what is the molecular compound.

i have tried it a little by making the mass of nitrogen 87.4 g. and found out the mass of hydrogen by subtracting 87.4 by 100. then i used the mass of each to find out the volume of each. then i used the ideal gas law for both nitrogen and hydrogen. this is all i did so far. i am not even sure if what i did is right. can you guys help me

 

[GCT]

Hello kevinf and welcome to PF. first use the ideal gas formula

PV=nRT

(n/V)=P/RT

n=total moles of the Nitrogen and Hydrogen gas

Found out how to convert the "total concentration to average density."

 

[Blueshift5]

Based on the information provided, it seems like you are on the right track. To determine the molecular formula of the compound, you will need to use the ideal gas law to calculate the number of moles of nitrogen and hydrogen in the sample. From there, you can use the molar ratios to determine the empirical formula of the compound. Then, you can use the molar mass of the compound to determine the molecular formula. It would also be helpful to double check your calculations and make sure all units are consistent. If you are still having trouble, I would recommend seeking assistance from a chemistry tutor or your instructor.