3. A mixture of ammonium phosphate ( and water, 50% ammonium phosphate by weight

Question

3. A mixture of ammonium phosphate ( and water, 50% ammonium phosphate by weight, flows into a tank at a rate of loo kg/minute. A second stream of pure water is flowing into the tank at a rate of 50 kg/minute. The tank was initially empty. The contents of the tank are well mixed. The flow rate out depends on time (measured in minutes), Denote the mass in the tank as and the mass of ammonium phosphate in the tank as 3.1 Write the overall mass balance equation and solve it. What is the mass in the tank after 1 hour? 3.2 Write the equation for the ammonium phosphate balance and solve it. How much ammonium phosphate is in the tank after one hour?

Explanation / Answer

First, write out the balanced equation (not always easy, but in this case, it is)
3 NH3 + H3PO4 -> (NH4)3PO4

looking at the stoiciometric coefficients, 1 mol of phosphoric acid forms 1 mol of ammonium phosphate.

You have 2.1g of H3PO4. H3PO4 has a molar mass of 98g/mol. therefore, you have 2.1g / 98 (g/mol) = 0.0215 mol of H3PO4.

Since this is the same number of mols of ammonium phosphate that will be produced by the reaction, there are 0.0215 mols of ammonium phosphate.

The molar mass of (NH4)3PO4 is 149 g/mol, so 0.0215 mol * 149 (g/mol) = 3.20 g

3.2g of ammonium phosphate will be formed from 2.1g of phosphoric acid

After one hour 3122kg of ammonium phosphate is left in the tank

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