Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 21, Problem 9QAP
Write the formulas of the following compounds.
(a) ammonia
(b) laughing gas
(c) hydrogen peroxide
(d) sulfur trioxide
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Chapter 21 Solutions
Chemistry: Principles and Reactions
Ch. 21 - Prob. 1QAPCh. 21 - Prob. 2QAPCh. 21 - Prob. 3QAPCh. 21 - Prob. 4QAPCh. 21 - Prob. 5QAPCh. 21 - Prob. 6QAPCh. 21 - Give the formula for the acidic oxide of (a) HNO3...Ch. 21 - Prob. 8QAPCh. 21 - Write the formulas of the following compounds. (a)...Ch. 21 - Prob. 10QAP
Ch. 21 - Prob. 11QAPCh. 21 - Prob. 12QAPCh. 21 - Prob. 13QAPCh. 21 - Prob. 14QAPCh. 21 - Prob. 15QAPCh. 21 - Prob. 16QAPCh. 21 - Prob. 17QAPCh. 21 - Write a balanced net ionic equation for the...Ch. 21 - Prob. 19QAPCh. 21 - Prob. 20QAPCh. 21 - Prob. 21QAPCh. 21 - Prob. 22QAPCh. 21 - Prob. 23QAPCh. 21 - Prob. 24QAPCh. 21 - Prob. 25QAPCh. 21 - Prob. 26QAPCh. 21 - Prob. 27QAPCh. 21 - Prob. 28QAPCh. 21 - Prob. 29QAPCh. 21 - Prob. 30QAPCh. 21 - Prob. 31QAPCh. 21 - Prob. 32QAPCh. 21 - Prob. 33QAPCh. 21 - Prob. 34QAPCh. 21 - The average concentration of bromine (as bromide)...Ch. 21 - Prob. 36QAPCh. 21 - Iodine can be prepared by allowing an aqueous...Ch. 21 - Prob. 38QAPCh. 21 - Prob. 39QAPCh. 21 - Prob. 40QAPCh. 21 - Prob. 41QAPCh. 21 - Prob. 42QAPCh. 21 - Prob. 43QAPCh. 21 - Prob. 44QAPCh. 21 - Prob. 45QAPCh. 21 - Given...Ch. 21 - What is the concentration of fluoride ion in a...Ch. 21 - Calculate the solubility in grams per 100 mL of...Ch. 21 - Prob. 49QAPCh. 21 - Follow the directions for Problem 49 for the...Ch. 21 - Consider the equilibrium system HF(aq)H+(aq)+F(aq)...Ch. 21 - Applying the tables in Appendix 1 to...Ch. 21 - Consider the reaction 4NH3(g)+5O2(g)4NO(g)+6H2O(g)...Ch. 21 - Data are given in Appendix 1 for white phosphorus,...Ch. 21 - Prob. 55QAPCh. 21 - Prob. 56QAPCh. 21 - Sodium hypochlorite is produced by the...Ch. 21 - Prob. 58QAPCh. 21 - Prob. 59QAPCh. 21 - Prob. 60QAPCh. 21 - Consider the reduction of nitrate ion in acidic...Ch. 21 - Prob. 62QAPCh. 21 - Choose the strongest acid from each group. (a)...Ch. 21 - Prob. 64QAPCh. 21 - Prob. 65QAPCh. 21 - Prob. 66QAPCh. 21 - Prob. 67QAPCh. 21 - Prob. 68QAPCh. 21 - Prob. 69QAPCh. 21 - Explain why (a) acid strength increases as the...Ch. 21 - Prob. 71QAPCh. 21 - Prob. 72QAPCh. 21 - The amount of sodium hypochlorite in a bleach...Ch. 21 - Prob. 74QAP
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- (3) HBrarrow_forwardwrite a balanced chemical equation for each (A) Iron (III) chloride reacts with sodium hydroxide to produce iron (III) hydroxide and sodium chloride. (B) Magnesium nitrite reacts with perchloric acid to produce magnesium perchlorate and nitrous acid. (C) Copper(II) hydroxide reacts with hydrosulfuric acid to produce copper (II) sulfide and water.arrow_forwardWrite a balanced formula equation for each of the following. Please answer parts (a) through (h) (a) Titanium metal reatcs with selenium to produce crystals of titanium(III) selenide. (b) Phosphoric acid is neutralized with barium hydroxide to produce a precipitate of barium phosphate in water. (c) Nitrogen gas reacts with lead(II) oxide powder to yield lead(II) nitride and oxygen gas. (d) Xenon hexafluoride crystals react with water to produce xenon trioxide powder and hydrofluoric acid. (e) Aluminum carbide is reacted with water in the synthesis of methane gas. Aluminum hydroxide precipitate is also formed. (f) Plants produce the simple sugar C6H12O6 and oxygen gas from carbon dioxide and water during photosynthesis. (g) Ammonia gas (NH3) is formed along with a precipitate of magnesium hydroxide from the reaction of magnesium nitride powder with water. (h) Strong heating of copper(II) nitrate trihydrate produces copper(II) oxide, nitrogen dioxide, oxygen gas and water.arrow_forward
- Write balanced equations for each of the following reactions.(a) When mercury(II) oxide is heated, it decomposesto form O2 and mercury metal. (b) When copper(II) nitrateis heated strongly, it decomposes to form copper(II) oxide,nitrogen dioxide, and oxygen. (c) Lead(II) sulfide, PbS(s),reacts with ozone to form PbSO4(s) and O2(g). (d) Whenheated in air, ZnS(s) is converted to ZnO. (e) Potassiumperoxide reacts with CO2(g) to give potassium carbonateand O2. (f) Oxygen is converted to ozone in the upperatmosphere.arrow_forwardWrite balanced equations for each of the following reactions(some of these are analogous to reactions shown inthe chapter). (a) Aluminum metal reacts with acids to formhydrogen gas. (b) Steam reacts with magnesium metal togive magnesium oxide and hydrogen. (c) Manganese(IV)oxide is reduced to manganese(II) oxide by hydrogen gas.(d) Calcium hydride reacts with water to generate hydrogengas.arrow_forward5.0g of solid zinc carbonate are heated to produce oxide and carbon dioxide. (a) Write a balanced chemical equation for the reaction. States are required. (b) Calculate the mass of carbon dioxide produced in the reaction.arrow_forward
- Hydrazine 1N2H42 and dinitrogen tetroxide 1N2O42 form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O. (a) Write a balanced chemical equation for this reaction.arrow_forwardWith the advent of techniques such as scanning tunneling microscopy, it is now possible to “write” with individual atoms by manipulating and arranging atoms on an atomic surface.(A) If the image is prepared on a platinum surface that is exactly 20 platinum atoms high and 14 platinum atoms wide, what is the mass (grams) of the atomic surface? Show all work. [2](B) If the atomic surface were changed to ruthenium atoms and the same surface mass as determined in part (B) is used, what number of ruthenium atoms is needed to construct the surface? Show all work. [2]arrow_forward4. Complete, formulate, and balance the following equations: (a) Calcium chloride + lead(II) nitrate (b) Sodium sulfide + zinc chloride (c) Barium hydroxide + Phosphoric acidarrow_forward
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