Please help me complete this two questions 3) Suppose you add 125g of C and 125g of Cl2 to an excess amount of TiO2, how muchTiCla can be produced according to the following reaction if the reaction has a percentage yieldof 73.8%.TiO:(s) + 2 Cl(g) + C(s) → TiCl,(1) + CO2 (g)4) What is the theoretical yield of calcium phosphate, Ca3(PO.)2 when 10.00 g of calciumhydroxide, Ca(OH); and 10.00 g of phosphoric acid, H;PO, are mixed according tothe following reaction.3Ca(OH) 2 (s) + 2H;PO4 (aq) → Cas(PO4) 2 (s) + 3H20 (1)

Answer :- (3) Mass (Practical yield) of TiCl4 = 123.4 g…

3) Suppose you add 125g of C and 125g of Cl; to an excess amount of TiO2, how much TiCla can be produced according to the following reaction if the reaction has a percentage yield of 73.8%. TiO(s) + 2 Cl,(g) + C(s) → TiCl(1) + CO; (g) 4) What is the theoretical yield of calcium phosphate, Ca,(PO,); when 10.00 g of calcium hydroxide, Ca(OH); and 10.00 g of phosphoric acid, H,PO, are mixed according to the following reaction. 3Ca(OH) 2 (s) + 2H3PO4 (aq) → Cas(PO.) 2 (s) + 3H;0 (1)

3) Suppose you add 125g of C and 125g of Cl; to an excess amount of TiO2, how much TiCla can be produced according to the following reaction if the reaction has a percentage yield of 73.8%. TiO(s) + 2 Cl,(g) + C(s) → TiCl(1) + CO; (g) 4) What is the theoretical yield of calcium phosphate, Ca,(PO,); when 10.00 g of calcium hydroxide, Ca(OH); and 10.00 g of phosphoric acid, H,PO, are mixed according to the following reaction. 3Ca(OH) 2 (s) + 2H3PO4 (aq) → Cas(PO.) 2 (s) + 3H;0 (1)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 81QRT: Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid...

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The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
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4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g)+3H2O(l)3CO(g)+7H2(g)
In an experiment designed to produce calcium oxide by the chemical reaction 2Ca + O2 2CaO 177.2 g of CaO was obtained out of a possible 203.9 g ofCaO. a. What is the theoretical yield of CaO? b. What is the actual yield of CaO? c. What is the percent yield of CaO?
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
Propane, C3H8, is the fuel of choice in a gas barbecue. When burning, the balanced equation is C3H8+5O23CO2+4H2O a What is the limiting reactant in cooking with a gas grill? b If the grill will not light and you know that you have an ample flow of propane to the burner, what is the limiting reactant? c When using a gas grill you can sometimes turn the gas up to the point at which the flame becomes yellow and smokey. In terms of the chemical reaction, what is happening?
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
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Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation? lf 2.50 moles of A2 are reacted with excess AB, what amount (moles) of product will form? If the mass of AB is 30.0 u and the mass of A2 are 40.0 u, what is the mass of the product? If 15.0 g of AB is reacted, what mass of A2 is required to react with all of the AB, and what mass of product is formed?
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
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