A process by which zirconium metal can be produced from the mineral zirconium (IV)orthosilicate, ZrSiO4, starts by reacting it with chlorine gas to form zirconium (IV)4»chloride.ZrSiO4 + 2 Cl2 → ZrCl4 + SiO2 + O2If 862 g ZrSiO4 and 950. g of Cl, are available, what is the limiting reactant (blank 1,no subscripts needed)? What is the mass of ZrCl4 (blank 2, no decimal places,rounded to the nearest 100)?

Answered: Image /qna-images/answer/d233773a-15ee-438d-a6aa-15ef0277189b.jpg

A process by which zirconium metal can be produced from the mineral zirconium (IV) orthosilicate, ZrSiO4, starts by reacting it with chlorine gas to form zirconium (IV) chloride. ZrSiO4 + 2 Cl2 → ZrC, + SiO2 + O2 If 862 g ZrSiO, and 950. g of Cl, are available, what is the limiting reactant (blank 1, no subscripts needed)? What is the mass of ZrCl4 (blank 2, no decimal places, rounded to the nearest 100)?

A process by which zirconium metal can be produced from the mineral zirconium (IV) orthosilicate, ZrSiO4, starts by reacting it with chlorine gas to form zirconium (IV) chloride. ZrSiO4 + 2 Cl2 → ZrC, + SiO2 + O2 If 862 g ZrSiO, and 950. g of Cl, are available, what is the limiting reactant (blank 1, no subscripts needed)? What is the mass of ZrCl4 (blank 2, no decimal places, rounded to the nearest 100)?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000°C and is used in welding metals: 2Al + Fe2O3 Al2O3 + 2Fe. In one process, 148 g of Al is reacted with 601 g of Fe₂O3. Calculate the mass (in grams) of Al2O3 formed, and determine the amount of excess reagent left at the end of the reaction. Mass of Al2O3 formed: g Amount of excess reagent: g of What is the limiting reactant?
Enter the coefficients directly from the balanced chemical equation. Do not reduce to lowest terms. For example: If 3 moles H, react with 3 moles O, enter "3" for each, not "1". According to the following reaction: 4HCI (aq) + 0, (g) 2H20 (1) + 2Cl, (g) What would you multiply "grams of hydrochloric acid" by to convert to the units "moles of oxygen" ? (number) (unit) (number) (unit) grams HCI = moles O2 (number) (unit) (number) (unit)
Enter the coefficients directly from the balanced chemical equation. Do not reduce to lowest terms. For example: If 3 moles H2 react with 3 moles 02, enter "3" for each, not "1". According to the following reaction: Ca(OH)2 (aq) + 2HCI (aq) –→ CaCl2 (aq) + 2H20 (1) What would you multiply "moles of calcium hydroxide" by to convert to the units "moles of water" ? (number) (unit) moles Ca(OH)2 = moles H20 (number) (unit)
Enter the coefficients directly from the balanced chemical equation. Do not reduce to lowest terms. For example: If 3 moles H2 react with 3 moles 02, enter "3" for each, not "1". According to the following reaction: 2Na (s) + 2H20 (I) –→ 2NaOH (aq) + H2 (g) What would you multiply "moles of sodium" by to convert to the units "moles of hydrogen" ? (number) (unit) = moles H2 moles Na (number) (unit)
The reaction between aluminum and iron(III) oxide (known as the thermite reaction) can generate temperatures approaching 3000 °C, and is used in welding metals: Al (s) + Fe2O3 (s) --> Al2O3 (s) + Fe (s) In one particular reaction, 124 g of Al are reacted with 601 g of Fe2O3. Calculate the mass (in grams) of Al2O3 that would be formed.
Determine the mass in grams of CO₂ that are produced by the complete reaction of 0.05090 moles of C₇H₈ (toluene) according to the following combustion reaction: C₇H₈(l)+ 9 O₂(g) → 7 CO₂(g) + 4 H₂O(g)
Consider the balanced chemical equation. What is the maximum number of gram Ag that can be produced if 0.570 mole of Zn and 0.691 mol of Ag2O react? Zn(s) + Ag2O(s) = ZnO(s) + 2Ag(s)
Dichlorine monoxide, Cl,0, is sometimes used as a powerful chlorinating agent in research. It can be produced by passing chlorine gas over heated mercury(I) oxide according to this equation: HgO+Cl2 → HgCl, + Cl20 What is the percent yield, if the quantity of reactants is sufficient to produce 8.90 g of Cl,0 but only 2.10 g is obtained? Answer in standard notation to the nearest tenth of a percent
One of the methods used to synthesize urea, (NH,,CO, is to react ammonia, NH,, with carbon dioxide, CO. The balanced reaction for this process is as follows: 2NH, + CO,(NH,),CO + H,0 Suppose we cary out this reaction by combining 7.481 g NH3 and 7.992 g CO, a What is the limiting reactant? b What will be the mass of the limiting reactant required?(only 3 decimal places) c. What are the moles of NH3 and CO2 ?(only 4 decimal places) mol NH3 mol CO d. How many moles of urea can be produced from the limiting reactant? (only 4 decimal places) mol (NHCO
Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P4(s) + 50₂(g) 2 P₂O5 (g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid (H₂PO4): P₂O₂(g) + 3H₂O(1) 2 H3PO4 (1) Suppose the yield of the first step is 94.% and the yield of the second step is 69.%. Calculate the mass of phosphorus required to make 8.0 kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Give a clear handwritten answer
Al2Cl6 is made by treating scrap metal with chlorine gas according to the following equation: 2 Al (s) + 3 Cl2 (g) ⟶⟶ Al2Cl6 (s) In the reaction of 45.9 g Al with 212.5 g Cl2, determine the limiting reactant and theoretical yield of the product. The limiting reactant is? The theoretical yield of Al2Cl6 is?. Round the answer to 1 decimal place. If the reaction produces 139.4 g Al2Cl6, calculate the percent yield of the reaction. ? %. Round the answer to 1 decimal place.