caculation:
2Na3PO4(aq)+3BaCl2(aq)-> 6NaCl(aq)+Ba3(PO4)2(s)
a)determine the maximum g of Ba3(PO4)2 that can be formed from your mass of Na3PO4x12H2O
b)determine the maximum gram of Ba(PO4)2 that can be formed from your mass of BaClx2H2O
To determine the maximum grams of Ba3(PO4)2 that can be formed (part a) and the maximum grams of Ba(PO4)2 that can be formed (part b), we need to calculate the limiting reagent in each case. The limiting reagent is the reactant that is completely consumed in the reaction and determines the amount of product that can be formed.
Before we start, we need to convert the given mass of Na3PO4·12H2O (in part a) and BaCl2·2H2O (in part b) into moles. To do this, we use the molar mass of each compound.
Step 1: Convert the mass of Na3PO4·12H2O into moles (part a):
- Determine the molar mass of Na3PO4·12H2O:
- 3(Na) = 3 * 22.99 g/mol = 68.97 g/mol
- 1(P) = 1 * 30.97 g/mol = 30.97 g/mol
- 4(O) = 4 * 16.00 g/mol = 64.00 g/mol
- 12(H) = 12 * 1.01 g/mol = 12.12 g/mol
- Total molar mass: 175.06 g/mol
- Convert the given mass of Na3PO4·12H2O into moles:
- Moles = Mass / Molar mass
- Moles of Na3PO4·12H2O = Mass of Na3PO4·12H2O / Molar mass of Na3PO4·12H2O
Step 2: Convert the mass of BaCl2·2H2O into moles (part b):
- Determine the molar mass of BaCl2·2H2O:
- 1(Ba) = 1 * 137.33 g/mol = 137.33 g/mol
- 1(Cl) = 1 * 35.45 g/mol = 35.45 g/mol
- 2(H) = 2 * 1.01 g/mol = 2.02 g/mol
- 2(O) = 2 * 16.00 g/mol = 32.00 g/mol
- Total molar mass: 206.80 g/mol
- Convert the given mass of BaCl2·2H2O into moles:
- Moles = Mass / Molar mass
- Moles of BaCl2·2H2O = Mass of BaCl2·2H2O / Molar mass of BaCl2·2H2O
Step 3: Calculate the moles of Ba3(PO4)2 that can be formed (part a):
- Based on the balanced equation, the mole ratio between Na3PO4 and Ba3(PO4)2 is 2:1.
- Moles of Ba3(PO4)2 = (Moles of Na3PO4·12H2O) * (1 mol Ba3(PO4)2 / 2 mol Na3PO4)
Step 4: Calculate the moles of Ba(PO4)2 that can be formed (part b):
- Based on the balanced equation, the mole ratio between BaCl2 and Ba(PO4)2 is 3:1.
- Moles of Ba(PO4)2 = (Moles of BaCl2·2H2O) * (1 mol Ba(PO4)2 / 3 mol BaCl2)
Step 5: Convert moles of Ba3(PO4)2 (part a) and Ba(PO4)2 (part b) into grams:
- Mass = Moles * Molar mass
Finally, let's plug in the values and calculate the results.