A 0.515 g sample of CaCl2 reacts with aqueous sodium phosphate to give 0.484 g Ca3(PO4)2. Sow the theorectical yield of Ca3(PO4)2.
3 CaCl2 + 2 Na3PO4 → Ca3(PO4)2 + 6 NaCl
Supposing there is excess sodium phosphate:
(0.515 g CaCl2) / (110.9840 g CaCl2/mol) x (1 mol Ca3(PO4)2 / 3 mol
CaCl2) x (310.1767 g Ca3(PO4)2/mol) =
0.4797 g Ca3(PO4)2 in theory
(0.484 g) / (0.4797 g) = 100.8 = 100.8 % yield
A 0.515 g sample of CaCl2 reacts with aqueous sodium phosphate to give 0.484 g Ca3(PO4)2....
8. A 0.700-g unknown mixture with CaCl2 reacts with aqueous sodium phosphate to give 0.425 8 Ca3(PO4)2. Refer to Example Exercise 15.2 and show the calculation for the percentage CaCl2 in the unknown mixture. DUTY in modo talentos Stan solo longo 9. What safety precautions must be observed in this experiment?
---Percent yield of Ca3(PO4)2 from CaCL2 Mass of beaker + CaCL2 = 342.231g, Mass of beaker = 341.852g, Mass of filter paper + Ca3(PO4)2 ppt = 0.726, Mass of filter paper = 0.506 1. Show the calculation for theoretical yield of Ca3(PO4)2 2. Show the calculation for percent yield of Ca3(PO4)2
A chemist fills a reaction vessel with 0.980 g calcium phosphate (Ca3(PO4)2) solid, 0.212 M calcium (Ca+2) aqueous solution and 0.119 M phosphate (PO4−3) aqueous solution at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy ΔG for the following chemical reaction: Ca3(PO4)2(s) 3Ca+2(aq)+2PO4−3(aq) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule.
2. 20.0 g of aqueous magnesium sulfate reacts with aqueous sodium phosphate and yields a soluble and an insoluble compound. (a) Write and balance the equation and indicate the physical state of reactants and products; (b) calculate the amount of insoluble product assuming more than enough sodium phosphate; and (c) find the number of moles of the insoluble product that can be obtained from 15.0 g sodium phosphate if there is more than enough of MgSO4. (25 points) (a) reaction...
DuPPY U111204) 20. Elemental phosphorous, P4, can be prepared by heating calcium phosphate, Ca3(PO4)2, with sand (silicon dioxide, SiO2) and coke (impure C). The balanced equation for this reaction is shown in Equation 18. d 2 Ca3(PO4), (s) + 6 SiO2(s) + 10C(s) + P (g) + 6 CaSiO3(s) + 10 CO(g) (Eq. 18) o What is th What is the percent yield of P, if 27.3 g of P4 are recovered from the reaction of 200 g of Ca3(PO4)2...
what is the molar solubility of Ca2+ in a 1.00 M aqueous solution of Ca3(PO4)2 (Ksp for calcium phosphate is 2.0 x 10^-29)
A volume of 50.0 mL of 0.0900 M CaCl2 reacts with excesss sodium carbonate to give 0.366 g of calcium carbonate precipitate. What is the percent yield?
Phosphoric acid can be prepared from calcium phosphate according to the following reaction: Ca3(PO4)2 (s) + 3 H2SO4 (l) → 3 CaSO4 (s) + 2 H3PO4 (l) 310. g/mol 98.0 g/mol 136 g/mol 98.0 g/mol [a] If 0.664 mole of Ca3(PO4)2 are combined with 1.53 mole of H2SO4, how many grams of H3PO4 can be produced? [4 pts] [b] If 62.6 g of H3PO4 is actually produced in the above reaction, what is the percent yield for the reaction? [2...
6.50 mol sodium phosphate completely reacts with magnesium chloride. 2Na3PO4 + 3MgCl2 ----> 6NaCl + Mg3(PO4)2 Show your work in calculating the amount of magnesium chloride that reacts.
Question 24 1 pts Write the solubility product constant expression for calcium phosphate, Ca3(PO4)2 O [Ca2+][PO43-M[Ca3(PO4)2] O Ca2+1*[PO43-12 O [Ca2+][PO43-1 O [Ca2+12[PO43-13