5. Part C. Single displacement, double displacement, and decomposition reactions may all be redox reactions. Identify the type of redox reactions in Part C. Explain. 6. Part C. a. On the basis of your intuitive understanding of the chemical properties.of sodium and gold, where in your activity series would you place sodium and gold? b. Will hydrochloric acid react with gold-metal to produce gold(I) ions and hydrogen gas? Explain.

5. Part C. Single displacement, double displacement, and decomposition reactions may all be redox reactions. Identify the type of redox reactions in Part C. Explain. 6. Part C. a. On the basis of your intuitive understanding of the chemical properties.of sodium and gold, where in your activity series would you place sodium and gold? b. Will hydrochloric acid react with gold-metal to produce gold(I) ions and hydrogen gas? Explain.

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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Chemical equations are written communications intended to describe chemical reactions happening before our eyes. a). What does the chemical equation for a synthesis reaction tell us is happening in the flask? b) What does the chemical equation for a decomposition reaction tell us is happening in the flask? Find and copy or write an example of a synthesis equation describing the formation of an ionic compound (a salt). d) For the product of this equation, write a chemical equation describing its decomposition. e) Choose an element that could react with your synthesis product to replace one of its ions. f) Explain how you chose this element and why you are certain it would react.
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MISSED THIS? Watch IWE: Writing Complete lonic and Net Ionic Equations ; Read Section 5.6. You can click on the Review link to access the section in your e Text. Lead ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution. contains lead(II) nitrate. K Part A Enter the complete ionic equation to show the reaction of aqueous lead (II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate. Express your answer as a chemical equation. Identify all of the phases in your answer. Submit ΑΣΦ A chemical reaction does not occur for this question. Part B ? Request Answer Review | Constants | Periodic Table Enter the net ionic equation to show the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate. Express your answer as a chemical equation. Identify all of the phases in your answer.
MISSED THIS? Watch KCV: Reactions in Solutions. IWE: Writing Equations for Acid-Base Reactions Involving a Strong Acid : Read Section 5.7. You can click on the Review link to access the section in your e Text. K ▾ Part A Enter balanced molecular equation for the reaction between nitric acid and magnesium hydroxide. Express your answer as a chemical equation including phases. 0 Submit Part B ΑΣΦ A chemical reaction does not occur for this question. 0 Request Answer Ć E ΑΣΦ Enter a net ionic equation for the reaction between nitric acid and magnesium hydroxide. Express your answer as a chemical equation including phases. ? www 1 ?
A precipitation reaction involves the formation of a precipitate when aqueous solutions are mixed. Not all combinations of aqueous solutions produce precipitates, and it is important to be able to predict the ones that do. A) Complete and balance the molecular equation for the reaction between aqueous solutions of lithium fluoride and potassium chloride, and use the states of matter to show if a precipitate forms. B) Write the complete ionic equation for the reaction that takes place when aqueous solutions of lithium fluoride and potassium chloride are mixed. C) Write the net ionic equation for the precipitation reaction, if any, that may occur when aqueous solutions of lithium fluoride and potassium chloride are mixed. If there is no net ionic equation, simply write "none."
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Write the molecular, complete, and net ionic reactions for aqueous lithium phosphate reacting with aqueous gold(III) nitrate to form solid gold(III) phosphate and aqueous lithium nitrate.a. molecular:b. complete:c. net:
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For each of the following sets of reactants, write the balanced equation for the single displacement reaction that occurs. If you determine that a reaction will not occur, write “NR”, and provide a brief explanation. a. Aluminum metal + aqueous nickel(II) nitrate b. Gold metal + hydrobromic acid
1. Would tin react with a copper (II) nitrate solution? Explain your answer and show any reaction that might oCcur. The Activity Series Lithium Potassium Barium These metals displace hydrogen from water Calcium Sodium Magnesium Aluminium Zinc Chromium Iron These metals displace hydrogen from acids. Cadmium Nickel Tin Lead Hydrogen Сopper Mercury Silver These metals do not displace hydrogen from Acids or water. Gold
B. Change these word equations into formula equations and balance them. Be sure to use the proper symbols to indicate the state of each substance, as given. 1. Upon heating, solid magnesium carbonate decomposes into solid magnesium oxide and carbon dioxide. 2. Solutions of Iron (III) sulfate and sodium hydroxide are mixed together, forming solid iron (III) hydroxide and a solution of sodium sulfate. 3. Gaseous sulfur trioxide reacts with liquid water to form a solution of sulfuric acid.
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. (Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit.) a. cobalt(III) chloride and sodium hydroxide b. silver nitrate and ammonium chromate c. copper(II) sulfate and lead nitrate d. calcium nitrate and sodium iodide +