Given the following reaction:  3AgNO3 (aq) + Na3PO4 (aq) => Ag3PO4 (s) + 3NaNO3 (aq) Suppose you have 2.25g of AgNO3 plus 1.25g of Na3PO4 produces 1.28g of solid.  What is the theoretical yield of silver phosphate (in grams)?   What is the percent yield of this reaction?

How many moles of NO₂ would be required to produce 3.34 moles of HNO₃ in the presence of excess water in the following chemical reaction? 3 NO₂(g) + H₂O (l) → 2 HNO₃(g) + NO(g)

Write the balanced NET ionic equation for the reaction when aqueous BaCl2 and aqueous (NH4)2SO, are mixed in solution to form aqueous NH,CI and solid BaSO4. O4- 3. 2. 2+ 3+ 4+ 1 2. 3 4 6. 7 8. 9. 4 7 8. 69 1. (s) (1) (g) (aq) Ba CI Reset • x H2O Delete SI 5.

Please help me fill in the blanks to find out theoretical yield

If you are given 1.35g Fe(NO3)3 and 0.00597 mol of Cl2 to conduct the gas forming reaction below 2Fe(NO3)3+2Cl2=2FeCl2+6NO2+3O2. What it's the limiting reagent? What is the theoretical yield of O2 formed in this reaction in moles. When the reaction was run only 0.00256 mol O2 are collected. What is the % yield for this process

If exactly 4.089 moles of propanol (C3H8O)  is combusted in the presence of excess oxygen what is the mass of O2 used in the reaction? The molecular weights of all reactants and products are: C3H8O: 60.09 g/mol O2: 31.998 g/mol H2O: 18.016 g/mol; CO2 : 44.01 g/mol. Enter your answer in the units of g, do not enter the unit itself.

(6)For the following balanced reaction use the mass of the chemical provided to solve the mass of the chemical asked for.  6 CO2 +  6 H2O  -->  1 C6H12O6   +   6 O2   202 g of CO2 is consumed by a plant undertaking this photosynthesis reaction.  Find the mass of C6H12O6 produced.

How many moles of NO₂ would be required to produce 4.62 moles of HNO₃ in the presence of excess water in the following chemical reaction? 3 NO₂(g) + H₂O (l) → 2 HNO₃(g) + NO(g)

One night you and your friend decided to help in agriculture. The farmer you are helping reacted 90 Kg of Calcium fluoride phosphate (Cas(PO4)3F) and 30L of sulfuric acid(H2SO4), so far he has collected 5Kg of hydrofluoric acid (HF) and the farmer wants to know the % yield of the HF to estimate the time needed to complete the reaction. Balance the equation, calculate the molecular weight and mols of Cas(PO4)3F and H2SO4 (Density of Sulfuric acid 1.84 g/cm3), Calculate the limiting reagent, the percent yield of HF and the number of molecules of so far. If the density of HF is 1.15 g/cm3 and the temperature of the 10 L vessel HF is contained is 25 C what is the pressure of the contained in which HF is collected? Ca(H2 PO4)2 (aq) + CaSO4 (aq) + HF (g) Cas(PO4)3F (s)+H2SO4 (aq)

How many moles of NO₂ would be required to produce 4.70 moles of HNO₃ in the presence of excess water in the following chemical reaction? 3 NO₂(g) + H₂O (l) → 2 HNO₃(g) + NO(g)