Concept explainers
Consider the unbalanced equation for the reaction of aluminum with sulfuric acid:
a. Balance the equation.
b. How many moles of
are required to completely react with 8.3 mol of AI?
c. How many moles of
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Chapter 8 Solutions
Introductory Chemistry, Books a la Carte Edition (5th Edition)
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Chemistry: A Molecular Approach (4th Edition)
Chemistry
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Inorganic Chemistry
Chemistry: The Central Science (13th Edition)
Chemistry: An Introduction to General, Organic, and Biological Chemistry (13th Edition)
- Balance the following equations representing combustion reactions: a. b. c. C12H22O11 (s) + O2(g) CO2 (g) + H2O (g) d. Fe(s) + O2(g) Fe2O3(s) e. FeO(s) + O2(g) Fe2O3(s)arrow_forward4.9 Sulfur, S8, combines with oxygen at elevated temperatures to form sulfur dioxide. (a) Write a balanced chemical equation for this reaction. (b) If 200 oxygen molecules are used up in this reaction, how many sulfur molecules react? (c) How many sulfur dioxide molecules are formed in part (b)?arrow_forwardHigh cost and limited availability of a reactant often dictate which reactant is limiting in a particular process. Identify the limiting reactant when the reactions below are run, and come up with a reason to support your decision. a. Burning charcoal on a grill: C(s)+O2(g)CO2(g) b. Burning a chunk of Mg in water: Mg(s)+2H2O(l)Mg(OH)2(aq)+H2(g) c. The Haber process of ammonia production: 3H2(g)+N2(g)2NH3(g)arrow_forward
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- Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.arrow_forwardNitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.arrow_forward3.16 Balance the following equations. (a) reaction to produce "super-phosphate" fertilizer: Ca3(PO4)2(s)+H2SO4(aq)( Ca(H2PO4)2(aq)+CaSO4(s) (b) reaction to produce diborane, B2H6: NaBH4(s) + H2SO4(aq) ( B2H6(g) + H2(g) + Na2SO4(aq) (c) reaction to produce tungsten metal from tungsten(VI) oxide: WO3(s)+ H2(g) ( W(s) + H2O(l) (d) decomposition of ammonium dichromate: (NH4)2Cr2O7(s)(N2(g)+H2O(l)+Cr2O3(s)arrow_forward
- Balance the following equations, and name each reactant and product: (a) SF4(g) + H2O() SO2(g) + HF() (b) NH3(aq) + O2(aq) NO(g) + H2O() (c) BF3(g) + H2O() HF(aq) + H3BO3(aq)arrow_forwardThe equation for the reaction of phosphorus and chlorine is P4(s) + 6 Cl2(g) 4 PCl3(). If you use 8000 molecules of P4, in this reaction how many molecules of C12 are required to consume the P4 completely?arrow_forward
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