reader6 - Chapter 4: Chemical Reactions 1, 5, 7, 9, 13, 15,...

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Chapter 4: Chemical Reactions 1, 5, 7, 9, 13, 15, 19, 21, 27, 29, 31, 37, 41, 43, 51, 53, 55, 59, 61, 63, 65, 71, 74 , 88 , 93 111, 112, 113 Writing and Balancing Chemical Equations 1.” Balance the following equations by inspection. (a) (b) (c) (d) 5.) Write balanced equations based on the information given. (a) (b) (c) (d) 7.” Write balanced equations to represent the complete combustion of (a) butane, C 4 H 10 ; (b) isopropyl alcohol, CH 3 CH(OH)CH 3 ; (c) lactic acid, CH 3 CH(OH)COOH. 9.” Write balanced equations to represent: (a) the decomposition, by heating, of solid ammonium nitrate to produce dinitrogen monoxide gas (laughing gas) and water vapor; (b) the reaction of aqueous sodium carbonate with hydrochloric acid to produce water, carbon dioxide gas, and aqueous sodium chloride;
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(c) the reaction of methane (CH 4 ), ammonia, and oxygen gases to form gaseous hydrogen cyanide and water vapor. Stoichiometry of Chemical Reactions 13.” Iron metal reacts with chlorine gas. How many moles of FeCl 3 are obtained when 7.26 mol Cl 2 reacts with excess Fe 15.” A laboratory method of preparing O 2 (g) involves the decomposition of KClO 3 (s). (a) How many moles of O 2 (g) can be produced by the decomposition of 32.8 g KClO 3 ? (b) How many grams of KClO 3 must be decomposed to produce 50.0 g O 2 ?
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(c) How many grams of KCl are formed, together with 28.3 g O2, in the decomposition of KClO3? 19.” The reaction of calcium hydride with water can be used to prepare small quantities of hydrogen gas, as is done to fill weather-observation balloons. (b)
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reader6 - Chapter 4: Chemical Reactions 1, 5, 7, 9, 13, 15,...

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