. A reaction of 220. mL of a lead (II) nitrate solution with excess hydroiodic acid produced 5.50 grams of solid lead (II) iodide and nitric acid. a. Determine the moles of lead (II) iodide produced b. Determine the moles of lead (II) nitrate that would react with the moles of lead (II) iodide calculated in part a.

. A reaction of 220. mL of a lead (II) nitrate solution with excess hydroiodic acid produced 5.50 grams of solid lead (II) iodide and nitric acid. a. Determine the moles of lead (II) iodide produced b. Determine the moles of lead (II) nitrate that would react with the moles of lead (II) iodide calculated in part a.

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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Two solutions are mixed, and the resulting reaction produces NaNO3(aq) and NiCO3(s). a. Write the balanced molecular equation for this reaction. b. Write the net ionic equation, given that the sodium and nitrate ions are the spectator ions.
Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct? a. Both KNO3 and NH4SO4 precipitate from solution b. A gad is released. c. KNO3 will precipitate from solution. d. NH4SO4 will precipitate from solution. e. No reaction will occur. Why is that answer "e"?
4. What are the types of ions and their respective molarities generated when following ionic compounds are dissolved in water to make aqueous solutions Solution Example: 1.5 M MgBr2 3.0 M Na₂S 2.0 M KNO3 Ions produced when dissolved in water One mole of Mg2+ ions are produced per every one mole of MgBr2 dissolved in water. Two moles of Br ions are produced per very one mole of MgBr2 dissolved in water. [One equivalent of Mg2+ and two equivalents (twice more) Br are produced.] Cation (+ ion) Molarity 1.5 M Mg Br₂ X 1 Mg²+ 1 MgBr2 = 1.5 M Mg2+ ions = Anion (-ion) Molarity 1.5 M MgBr₂ X 2 Br 1 MgBr₂ 3.0 M Br ions
3. What mass of NaCl can be produced from 0.55 mol Cl2 in the following reaction? 2 Naa + Cle) → 2 NaCle) d. 88 g a. 0.55 g b. 1.1 g с. 64 g С.
4. H₂S (aq) + Reaction type: 5. CaCO3 (s)→ CO₂ (g) + Reaction type: 6. C4H10O (g) + O₂(g) → Reaction type: 7. Ss (s) + Reaction type: 8. H₂SO4 (aq) + Reaction type: AsCl3 (aq) →__ AS2S3 (s) + Fe (s) → 9. H3PO4 (aq) + Reaction type: Al (s) → CaO (s) CO₂ (g) + FeS (s) _Al2(SO4)3 (aq) + NH4OH (aq) → HCI (aq) H₂O (e) - H₂(g) (NH4)3PO4 (aq) + HOH (e)
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.
1. CuSO4 a. copper(l) sulfate b. copper sulfate C. copper(II) sulfate d. copper sulphide 2. Nal a. sodium iodide C. sodium monoiodide b. sodium(1) iodide d. sodium iodate
The great French chemist Antoine Lavoisier discovered the law of conservation of mass in part by doing a famous experiment in 1775. In this experiment they found that mercury(II) oxide, when heated, decompose into liquid mercury and an invisible and previously unknown substance: oxygen gas. A. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury (II) oxide (HgO) into liquid mercury and gaseous dioxygen. B. Suppose 72 mL of dioxygen gas are produced by this reaction, at a temperature of 120°C and pressure of exactly 1 atm. Calculate the mass of mercury (II) oxide that must have reacted in grams. Round your answer to three significant digits.
8. Write balanced chemical equations for the following reactions. a. The reaction of gaseous homonuclear diatomic nitrogen and gaseous homonuclear diatomic hydrogen to produce gaseous ammonia, NH3. b. The reaction of solid manganese(IV) oxide and gaseous hydrogen chloride to produce solid manganese(lI) chloride, homonuclear diatomic chlorine gas, and water.
A. Which group 3 element is the most reactive? Express your answer as a chemical symbol. B. An oxide of a group 4 element is commonly used as a white pigment in paints, paper, rubber, and plastic and is accepted as the most important compound of the group 4 elements. Identify this compound. Express your answer as a chemical formula. C. What is the most common oxidation state of the group 5 elements? the oxidation state: D.A group 6 element (MM) is in a compound with the formula MBr2. The same metal forms a red solid with the formula MO3. What is the identity of MM? Express your answer as a chemical symbol.
Which of the following is a precipitation reaction? a. None are precipitation reactions. b. Two of the reactions are precipitation reactions. O . AGNO3(aq) + NaCl(aq) – O d. CaCl2(aq) + K2CO3(aq) – e. CO(g) + PbO(s) - Cl2(aq) + 21(aq) – O g. Pb(OH)2(s) –
Consider the following reaction:2HCl+CaCO3→CaCl2+H2O+CO22HCl+CaCO3→CaCl2+H2O+CO2How many mols of calcium chloride can be produced if you begin with 14.47 mL of 0.62 M HCl and 7.24 grams of calcium carbonate?