What volume of N2O (s) will be generated if 3.13 g of NH4NO3 (s) decomposes at 1.00 atm and 50 degrees celsius, given the following decomposition reaction: NH4NO3 (s) --> N2O (g) + 2 H2) (l)?

Answer 1

Here is how you work a stoichiometry problem.
1. Write and balance the equation. You have that.

2. Convert what you have (in this case grams NH4NO3) to mols. mols = grams/molar mass = ?

3. Using the coefficients in the balanced equation, convert mols of what you have to mols of what you want(in this case N2O).
mols N2O = ?mols NH4NO3 x (1 mol N2O/1 mol NH4NO3) = ?

4. Now convert mols N2O at the conditions listed with PV = nRT.
(NOTE: If you wanted grams N2O instead it would be grams N2O = mols N2) x molar mass N2O = ?

Print this out. It will work all of your stoichiometry problems. It's just a four step process.