Phosphoric acid, H3PO4 (aq), is used to make fertilizers and is present in cola drinks. Phosphoric acid can be prepared in a two-step process: P4+502-P4010 P4O10+ 6H₂O 4H;PQA - We allow 272 g of phosphorus to react with excess oxygen to form tetraphosphorus decaoxice, P4010, in 89.5% yield. In the 2nd reaction, a 96.8 % yield of H3PO4 (aq) is obtained. What is the mass of H₂PO4 (aq) obtained?

Lead(II) carbonate, also called "white lead," was formerly used as a pigment in white paints. However, because of its toxicity, lead can no longer be used in paints intended for residential homes. Lead(II) carbonate is prepared industrially by reaction of aqueous lead(II) acetate with carbon dioxide gas. The unbalanced equation is Pb(C,H3 O2)2 (ag) + H2O(1) + CO2(9) → PbCO3(s) + HC,H3 O2 (ag) Suppose an aqueous solution containing 1.20 g of lead(II) acetate is treated with 5.85 g of carbon dioxide. Calculate the theoretical yield of lead carbonate. Theoretical yield = g PbCO3

00 S Nazza .01608 ·018302 3. (part a). You are given 0.104 g of a sample of KwFex(C₂O4)y(H₂O)z. In the laboratory, you titrate this sample with 0.00940 M KMnO4 and you need 10.1 mL of the KMnO4 solution to reach the stoichiometric point. Calculate the mass and moles of [C₂04]²- in the sample. Please show all of your detailed calculations.

Chlorine gas can be produced in the laboratory by adding concentrated hydrochloric acid, HCl, to manganese(IV) oxide according to the following reaction: MnO2 (s)   +   4 HCl (aq)   →   MnCl2 (aq)   +   2 H2O (l)   +   Cl2 (g) What mass of MnO2 is required to produce 48.4 g Cl2 by the following reaction? Be sure to enter a unit with your answer.

2HCN(9) + 6H,0 2NH3 (9) 302(9) (g) ----- ----- + + 2CH4 (9) 4. How many Liters of HCN gas can form from the reaction of 1.56 x 10° grams of NH3, 4.5 moles of oxygen gas, and 12.2 Liters of methane gas? What mass of excess reactant remains?

6. Consider the following chemical reaction: 2 Cr(OH)3(aq) >Cr₂O3(s) + 3H₂0(1) 12.00 moles of chromium (III) hydroxide is decomposed. Calculate moles of the water produced. O 18.00 moles O 1.500 moles O 4.00 moles O 12.00 moles

Balance the following equations in which ethane, C2H6, burns in oxygen.    C2H6(g) + O2(g) --> C(s) + H2O(g)    C2H6(g) + O2(g) --> CO(g) + H2O(g)    C2H6(g) + O2(g) --> CO2(g) + H2O(g) d.   Explain why the coefficients for oxygen vary, depending on whether C, CO, or CO2 is formed.

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Lead (II) carbonate, also called "white lead," was formerly used as a pigment in white paints. However, because of its toxicity, lead can no longer be used in paints intended for residential homes. Lead(II) carbonate is prepared industrially by reaction of aqueous lead(II) acetate with carbon dioxide gas. The unbalanced equation is Pb(C₂H3O2)2 (aq) + H₂O(l) + CO₂(g) PbCO3(s) + HC₂H3 O2 (aq) Suppose an aqueous solution containing 1.15 g of lead (II) acetate is treated with 5.80 g of carbon dioxide. Calculate the theoretical yield of lead carbonate. Theoretical yield = g PbCO3

Iodine is prepared both in the laboratory and commercially by adding Cl2(g) to an aqueous solution containing sodium iodine 2Nal(aq)+Cl2(g)---> I2(s)+2NaCl(aq)  How many grams of sodium iodide, NaI, must be used to produce 82.1 g of iodine, I2?