4) A 11.31 g sample of a competitor's "SonicBloom" fertilizer is analyzed for its phosphorus content by gravimetric analysis through a reaction with magnesium sulfate and ammonia in water. The resulting MGNH4PO4 · 6H2O precipitate was dried and had a mass of 7.11 g. a) How many moles of phosphorus atoms are in the fertilizer sample? b) What is the weight percentage of phosphorus atoms in the fertilizer? c) What is the weight percentage of P2O5 in the fertilizer? (Or in other words, what was its middle N-P-K number?)

83. The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and cal- culate how many kilograms of carbon dioxide are added to the atmosphere per 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

Please don't provide handwritten solution ....

Write a balanced chemical equation based on the following description: liquid C₇H₈O is burned with oxygen gas to produce gaseous carbon dioxide and water vapor

The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO,(G) + 0,(g) 2M1O,(G) + 2C0, (g) In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO, (s) + 4Al(s) 3 Mn(s) + 2 Al,O3 (s) Suppose the yield of the first step is 95.% and the yield of the second step is 84.%. Calculate the mass of manganese(II) carbonate required to make 10.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. olo

Explain the term "limiting reactant". What is an ionic equation? Explain the meaning of "the reaction goes to less than 100% completion".

1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction.  b) What mass of acetic acid is in the aqueous solution?  c) Which of the reactants is the limiting reagent? Justify your answer.  d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction?  f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container?      please answer d, e and f

In a double replacement reaction, 1.214 g of tin(ii) fluoride react with sodium phosphate to form a precipitate. If the tin (ii) phosphate precipitate weighs 1.078 g, what is the percent yield?

An aqueous solution of NaF and an aqueous solution of PbCl2 react. Predict what solid will form and balance the chemical equation. If 30.6 mL of NaF solution reacted completely with excess PbCl2 to produces 10.7 g of the precipitate. What is the molarity of the original NaF solution?

(b) An unknown mass of Na3PO4(s) is dissolved in water to form 50.00 mL of solution. This is Solution A. Then 10.00 mL of Solution A is diluted with water to 50.00 mL. The final solution is Solution B. 20.00 mL of Solution B contains 4.408 x 1020 sodium ions. (NA = 6.022 x 1023 mol-1) Calculate the mass of Na3PO4(s) that was dissolved to form Solution A.