ResourcesO HintCheckGeneral Chemistry 4th Edition.McQuarrie Rock GalloglyUniversity Science Bookspresented by Macmillan LeamingCryolite, Na, AIF,(s), an ore used in the production of aluminum, can be synthesized using aluminum oxide.Balance the equation for the synthesis of cryolite.equation: AL,O, (s) + NaOH(I) + HFg)Na, AIF, + H,O(g)If 14.4 kg of Al, 0,(s), 57.4 kg of NaOH(1), and 57.4 kg of HF(g) react completely, how many kilograms of cryolite willbe produced?kg Na, AlF,nass of cryolite produced:Which reactants will be in excess?O HFNaOHO Al,0,What is the total mass of the excess reactants left.over after the reaction is comnlete?

The reaction taking place is given as, => Al2O3 (s) + NaOH (l) + HF (g) -------> Na3AlF6 (s) +…

Cryolite, Na, AlIF, (s), an ore used in the production of aluminum, can be synthesized using aluminum oxide. Balance the equation for the synthesis of cryolite. equation: AL,0, (s) + NaOH(1) + HFg) → Na, AIF, + H,O(g) If 14.4 kg of Al,0,(8), 57.4 kg of NaOH(), and 57.4 kg of HF(g) react completely, how many kilograms of cryolite will be produced? nss of cryolite produced: kg Na, AIF, Which reactants will be in excess? HF O NAOH O Al,0, What is the total mass of the excess reactants left.over after the reaction is comnlete?

Cryolite, Na, AlIF, (s), an ore used in the production of aluminum, can be synthesized using aluminum oxide. Balance the equation for the synthesis of cryolite. equation: AL,0, (s) + NaOH(1) + HFg) → Na, AIF, + H,O(g) If 14.4 kg of Al,0,(8), 57.4 kg of NaOH(), and 57.4 kg of HF(g) react completely, how many kilograms of cryolite will be produced? nss of cryolite produced: kg Na, AIF, Which reactants will be in excess? HF O NAOH O Al,0, What is the total mass of the excess reactants left.over after the reaction is comnlete?

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...

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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: P,(s) + 50,(g) 2 P,0; (g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid (H,PO,): P,0;(g) + 3H,0(1) 2 H;PO, (1) Suppose the yield of the first step is 77.% and the yield of the second step is 67.%. Calculate the mass of phosphorus required to make 6.0 kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water?Include the appropriate number of significant figures in your answer. 2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1. What is the percent yield of this reaction?Report your answer to the correct number of significant figures. 3)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na2CO3 does this solution contain? Express your answer to the correct number of significant figures. 4)Suppose the Na2CO3 solution described in Question 3 is added to a solution that contains excess CaCl2? What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction?…
Aspirin can be synthesized in the lab by combining salicylic acid (C,H,0,) and acetic anhydride (C,H,0,) to form aspirin ( C,H,O.) and acetic acid (C,H,O,). The balanced equation for this reaction is C,H,0, + C,H,O, → C,H,0, + C,H¸0, A student started with 3.33 mL acetic anhydride (density = 1.08 g/mL) and 2.61 g salicylic acid. The student synthesized 2.53 g of aspirin. Select the limiting reactant. salicylic acid (C,H,O,) acetic anhydride (C,H,0,) aspirin (C, H,O,) acetic acid (C,H0,) Calculate the theoretical yield of aspirin (C,H, O,). theoretical yield: uloto the percent yield for aspirin (C, H, O).
1. Balance the reaction equations below. a) HCl(aq) + _Mg(OH)2(s) – Н-0() + MgCl2(aq) b) _HNO3(aq) + Na,S(aq) → _H,S(g) + NANO3(aq) 2. What is the moles HCI-to-moles MgCl2 ratio in reaction (a)?
1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water?Include the appropriate number of significant figures in your answer. 2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1. What is the percent yield of this reaction?Report your answer to the correct number of significant figures. 3)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na2CO3 does this solution contain? Express your answer to the correct number of significant figures. 4)Suppose the Na2CO3 solution described in Question 13 is added to a solution that contains excess CaCl2? What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction?…
The rocket boosters of the space shuttle Discovery, launched on July 26, 2005, used a fuel mixture containing primarily solid ammonium perchlorate, NH4ClO4, and aluminum metal. The unbalanced chemical equation for the reaction is given below. (Hint: Balance the elements in the order Cl, H, O, Al, N.) Al(s) + NH4CIO4(s) Al₂O3(s) + AlCl3(s) + H₂O(l) + N₂(g) What is the mass (in kilograms) of NH4ClO4 consumed per kilogram of Al, assuming a percent yield of 87.20%? (Answer with two decimal places.)
Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide: 2 MnCO3(s) + O₂(g) 2 MnO₂ (s) +2 CO₂(g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide: 3 MnO₂(s) +4 Al(s)-3 Mn(s) +2 Al₂O3(s) Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced. ol 41
Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite. involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide: 2 MNCO,(s)-0,(g)→2 MnO,(s)-2 C0 (g) In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide: 3 MnO, (s)- 4 Al(s)-3 Mn(s)–2 Al,O,(s) Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced.
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: 2MnCO3(s) + O₂(g) → In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO₂ (s) + 4A1(s) 3 Mn (s) + 2 Al₂O3(s) Check 2 MnO₂ (s) + 2 CO₂ (g) Suppose the yield of the first step is 88.% and the yield of the second step is 70.%. Calculate the mass of manganese(II) carbonate required to make 1.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. 0 0 x10 nin 0 0.0 S Save For Later E OL A S C Submit Assignmen
4.) 325 g of H2O is poured onto a 450. g block of sodium metal. The equation for this reaction is: Na + H2O – - NaOH + H2 What is the limiting reactant?
Complete and balance the molecular equation for the reaction of aqueous copper(II) chloride, CuCl2, and aqueous potassium phosphate, K3PO4. Include physical states. molecular equation: CuCl₂(aq) + K3PO4 (aq) - Enter the balanced net ionic equation for this reaction. Include physical states. net ionic equation:
* CO (be • Part C Na + HCI→ Express your answer as a balanced equation including states of matter. Write "NR" if no reaction occurs. P3V 2Na(s) + 2HC1(g)→2NaCl(aq) + H, (g) Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Part D Na + Ca2+ Express your answer as a balanced equation. Do not include states of matter. Write "N.R." if no reaction occurs. DA chemical reaction does not occur for this question. Submit Request Answer Provide Feedback P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy Permi G Search or type URL %23 %$4 i 4. 5. 3. F.