Question
When heated to 350. ∘C at 0.950 atm, ammonium nitrate decomposes to produce nitrogen, water, and oxygen gases:
2NH4NO3(s)→Δ2N2(g)+4H2O(g)+O2(g)
Using the ideal gas law equation, calculate the volume, in liters, of water vapor produced when 21.8 g of NH4NO3 decomposes.
2NH4NO3(s)→Δ2N2(g)+4H2O(g)+O2(g)
Using the ideal gas law equation, calculate the volume, in liters, of water vapor produced when 21.8 g of NH4NO3 decomposes.
Answers
1. mols NH4NO3 = grams/molar mass = ?
2. Using the coefficients in the balanced equation, convert mols NH4NO3 to mols H2O.
3. Now use PV = nRT, substitute mols from above for n, use the conditions of P and T in the problem, solve for V in liters. Remember to change 350 C to kelvin.
Post your work if you get stuck.
2. Using the coefficients in the balanced equation, convert mols NH4NO3 to mols H2O.
3. Now use PV = nRT, substitute mols from above for n, use the conditions of P and T in the problem, solve for V in liters. Remember to change 350 C to kelvin.
Post your work if you get stuck.
im very stuck on finding r
Does V=188.4 L?
Just kidding. I mean 51.34L?