Sulfuric acid dissolves aluminum metal according to the following reaction: 2 Al(s) + 3 H2SO4(aq) + Al2(SO4)3(aq) + 3 H2(8) What minimum mass of H2SO4 would you need? Suppose you wanted to dissolve an aluminum block with a mass of 15.7 g. Express your answer in grams. TempBes Symbols uado redo resat keyboard shortcuts help Submit Request Answer Part B What mass of H2 gas would be produced by the complete reaction of the aluminum block? Express your answer in grams. TempBes Symbols uado redo resat keyboard shortcuts help, m%3D

Sulfuric acid dissolves aluminum metal according to the following reaction: 2 Al(s) + 3 H2SO4(aq) + Al2(SO4)3(aq) + 3 H2(8) What minimum mass of H2SO4 would you need? Suppose you wanted to dissolve an aluminum block with a mass of 15.7 g. Express your answer in grams. TempBes Symbols uado redo resat keyboard shortcuts help Submit Request Answer Part B What mass of H2 gas would be produced by the complete reaction of the aluminum block? Express your answer in grams. TempBes Symbols uado redo resat keyboard shortcuts help, m%3D

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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One can make a silver penny by plating silver onto older (pre-1982) copper pennies according to the following reaction. Cu(s) + 2 AgNO3(aq) 2 Ag(s) + Cu(NO3)2(aq) 1.27 grams of Copper were added to a solution that contains 5.10 grams of AgNO3. What many moles of Copper (II) nitrate would you expect at the end of the reaction
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Suppose 0.0350 g Mg is reacted with 10.00 mL of 6 M HCI to produce aqueous magnesium chloride and hydrogen gas. Mg(s) + 2HC1(aq) → MgCl2(aq) +H2(g) What is the limiting reactant in this reaction? Select one: Magnesium metal Hydrochloric acid Magnesium chloride Hydrogen gas
2.The following reaction takes place as represented by the balanced chemical equation below: 2 K3PO4 (aq) + 3 Ba(NO3)2 (aq) --> 6 KNO3 (aq) + Ba3(PO4)2 104.7 mL of a 2.50 M K3PO4 solution is reacted with an excess amount of Ba(NO3)2 solution. How many grams of Ba3(PO4)2 should be produced? Numerical answer: Unit: Label: Ba3(PO4)2
The balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous Nal is shown below. Pb(ClO3)2(aq) + 2 NaI(aq) → PbI2 (s) + 2 NaClO3(aq) What mass of precipitate will form if 1.50 L of excess Pb(ClO3)2 is mixed with 0.400 L of 0.100 M NaI? Assume 100% yield and neglect the slight solubility of PbI2.
Solution Stoichiometry A 25.0 ml sample of 1.20 M KCI solution is mixed with 15.0 mL of 0.900 M Pb(NO3)2 solution and the following precipitation reaction occurs: 2 KCI(aq) + Pb(NO3)2(aq) D PbC12(s) + 2 KN03(aq) The solid lead(II) chloride is collected, dried, and found to have a mass of 2.45 g. Determine the percent yield of lead(II) chloride.
The following reaction takes place as represented by the balanced chemical equation below: 2 K3PO4 (aq) + 3 Ba(NO3)2 (aq) --> 6 KNO3 (aq) + Ba3(PO4)2 104.7 mL of a 2.50 M K3PO4 solution is reacted with an excess amount of Ba(NO3)2 solution. How many grams of Ba3(PO4)2 should be produced? Numerical answer: Unit: Label: Ba3(PO4)2
In the following reaction, 35.0 mL of 0.150 M magnesium bromide solution reacts with excess silver nitrate to form a precipitate. What is the expected mass of AgBr in grams? (molar mass of AgBr = 187.77 g/mole) MgBr2(aq) + 2AgNO3(aq) --> 2AgBr(s) + Mg(NO3)2(aq) Question 11 options: 0.985 g 0.493 g 1.97 g 986 g none of these
I chose 99% was I right other options were 1% 51% 25%
Excess silver(I) nitrate was added to a 8.500 g mixture containing some amount of barium chloride, and 6.025 g of silver chloride was obtained. The unbalanced equation is AgNO3(aq) + BaCl2(aq) --> Ba(NO3)2(aq) + AgCl(s). What is the mass% of BaCl2 in the mixture?
Name: Section: Report Sheet (Data must be recorded directly in pen) Write the balanced chemical equation for the reaction of copper (II) sulfate and aluminum 3 CuSO4 + 2Al(s) → 1 Al₂(SO4) = (aq) + 3 Cu (s) DETERMINE THE LIMITING REACTANT. Show your calculations of starred items on next page Volume of CuSO4: 50.0 mL. 0.0500 L Molarity of CuSO4 used: 1.00 "Moles of CuSO4 used: 0.0500 0.0500 "Moles of copper produced based on CuSO, used: Molar mass of copper: *Grams of copper produced based on CuSO4 used: Mass of aluminum used Molar mass of aluminum "Moles of aluminum used: "Moles of copper produced based on Al used: Molar mass of copper: *Grams of copper produced based on Al used: Aluminum Limiting Reagent: Theoretical Yield: Actual Yield: "Percent Yield: g Cu Date: g Cu % yield Cu 63.546 318 0.759 26.982 - M CuSO4 moles CuSO moles Cu g/mol Cu(Periodic Table) g Cu g Al g/mole Al Pericdit Table D. 0281 moles of Al 0.0422 moles Cu 63.546 g/mol Cu (periodic table) 2.48 g Cu
When an ionic solid dissolves in water, water molecules attract the ions causing them to dissociate orcome apart. The resulting dissolved ions are electrically charged particles that allow the solution toconduct electricity. The following chemical equations represent this phenomenon:NaCl (s) → Na+ (aq) + Cl-(aq)Na2CO3 (s) → 2Na+(aq) + CO32- (aq)Write a similar balanced chemical equation for the other four strong electrolytes in the data table NaHCO3 KNO3NH4Cl HCl