What is the mass of nitrogen in 43.7 g of ammonium carbonate, (NH4)2CO3?

Sure, let's break this down:

1. First, we need to find the molar mass of ammonium carbonate, (NH4)2CO3. The molar mass is calculated by adding up the molar masses of all the atoms in the compound.

   • Nitrogen (N) has a molar mass of 14.01 g/mol. Since there are two nitrogen atoms in ammonium carbonate, the total mass of nitrogen is 2 * 14.01 = 28.02 g/mol.
   • Hydrogen (H) has a molar mass of 1.01 g/mol. Since there are eight hydrogen atoms in ammonium carbonate, the total mass of hydrogen is 8 * 1.01 = 8.08 g/mol.
   • Carbon (C) has a molar mass of 12.01 g/mol. Since there is one carbon atom in ammonium carbonate, the total mass of carbon is 12.01 g/mol.
   • Oxygen (O) has a molar mass of 16.00 g/mol. Since there are three oxygen atoms in ammonium carbonate, the total mass of oxygen is 3 * 16.00 = 48.00 g/mol.

   Adding these up, the molar mass of ammonium carbonate is 28.02 + 8.08 + 12.01 + 48.00 = 96.11 g/mol.

2. Next, we need to find the mass fraction of nitrogen in ammonium carbonate. This is done by dividing the total mass of nitrogen by the molar mass of ammonium carbonate.

   • The mass fraction of nitrogen is 28.02 g/mol / 96.11 g/mol = 0.291.

3. Finally, we can find the mass of nitrogen in 43.7 g of ammonium carbonate by multiplying the mass of the sample by the mass fraction of nitrogen.

   • The mass of nitrogen is 43.7 g * 0.291 = 12.7 g.

So, the mass of nitrogen in 43.7 g of ammonium carbonate is approximately 12.7 g.