To determine the amount of water produced when 50 grams of ammonium nitrate (NH4NO3) decomposes, we can use the balanced chemical equation:
NH4NO3 → N2 + O2 + H2O
We are given that 24 grams of nitrogen gas (N2) and 12 grams of oxygen gas (O2) are produced. To find the amount of water (H2O) produced, we need to calculate the remaining mass of water.
The molar mass of nitrogen gas (N2) is 28 grams/mol, and the molar mass of oxygen gas (O2) is 32 grams/mol. By calculating the number of moles of nitrogen and oxygen produced, we can determine the ratio between nitrogen, oxygen, and water in the balanced equation.
Moles of nitrogen gas (N2):
24 g N2 * (1 mol N2 / 28 g N2) = 0.857 mol N2
Moles of oxygen gas (O2):
12 g O2 * (1 mol O2 / 32 g O2) = 0.375 mol O2
Since the balanced equation shows that the ratio between nitrogen gas, oxygen gas, and water is 1:1:1, the moles of water produced will be the same as the moles of nitrogen and oxygen.
Moles of water (H2O):
0.857 mol H2O (water)
0.375 mol H2O (water)
To calculate the mass of water, we multiply the moles of water by the molar mass of water (18 grams/mol).
Mass of water (H2O):
0.857 mol H2O * (18 g H2O / 1 mol H2O) = 15.426 grams of water
0.375 mol H2O * (18 g H2O / 1 mol H2O) = 6.75 grams of water
Therefore, when 50 grams of ammonium nitrate decomposes, it produces approximately 15.426 grams of water.