The following thermochemical equation is for the reaction of NH4NO3 to form N2O and H2O.
NH4NO3 -> N2O+2H2O ΔH°=-35.9kj
How many grams of NH4NO3 would have to react to produce 10.4 kJ of energy?
_________grams
Guide On Rating System
Vote
To determine how many grams of NH4NO3 would have to react to produce 10.4 kJ of energy, we need to use the given enthalpy change (ΔH°) and the molar mass of NH4NO3.
First, let's calculate the molar mass of NH4NO3:
Molar mass of NH4NO3 = (1 * molar mass of N) + (4 * molar mass of H) + (3 * molar mass of O)
= (1 * 14.01 g/mol) + (4 * 1.01 g/mol) + (3 * 16.00 g/mol)
= 80.05 g/mol
Next, let's calculate the number of moles of NH4NO3 required to produce 10.4 kJ of energy:
ΔH = -35.9 kJ
ΔH per mole of NH4NO3 = -35.9 kJ/mol
Number of moles of NH4NO3 = (Energy required / ΔH per mole of NH4NO3)
= (10.4 kJ / -35.9 kJ/mol)
Finally, let's calculate the mass of NH4NO3 in grams:
Mass of NH4NO3 = (Number of moles of NH4NO3) * (molar mass of NH4NO3)
= ((10.4 kJ / -35.9 kJ/mol) * (80.05 g/mol)
The mass of NH4NO3 required to produce 10.4 kJ of energy is approximately 23.8 grams.
Got a question with my answer?
Cheapmath.com is completely free!
Asking question is free.
Getting answers is free.
+99