Answer :
Final answer:
The number of moles of nitrogen atoms in 51.7 g of ammonium nitrate is calculated by first finding the molar mass of ammonium nitrate. Then using the formula (moles = mass/molar mass), the moles of ammonium nitrate is calculated, which is then multiplied by 2 to get the total moles of nitrogen atoms. In 51.7 g of ammonium nitrate, there are approximately 1.2925 moles of nitrogen atoms.
Explanation:
To answer your question about how many moles of nitrogen atoms are in 51.7 g of ammonium nitrate, we first need to determine the molar mass of ammonium nitrate. Ammonium nitrate, NH4NO3, has 2 nitrogen atoms, 4 hydrogen atoms and 3 oxygen atoms. Using the atomic masses from the periodic table, nitrogen is approximately 14 g/mol, hydrogen is approximately 1 g/mol, and oxygen is approximately 16 g/mol.
Calculating the molar mass of ammonium nitrate (NH4NO3), we get: (2 * 14 g/mol) + (4 * 1 g/mol) + (3 * 16 g/mol) = 80 g/mol
To calculate the moles of nitrogen atoms in the given mass of ammonium nitrate, use the formula: moles = mass/molar mass. So, moles of NH4NO3 = 51.7 g ÷ 80 g/mol = 0.64625 mol.
Since there are two moles of nitrogen atoms in every mole of ammonium nitrate, you just multiply this result by 2 to get total moles of nitrogen: 2 * 0.64625 mol = 1.2925 moles of nitrogen atoms.
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