For each of the following balanced equations, write theoxidation number above the symbol of each atom thatchanges oxidation state in the course of the reaction.(a) N,O4(g) + KCI(s) → NOCI(g) + KNO3(s)(b) H,S(g) + 4 O̟F2(s) –(c) 2 POB13(s) + 3 Mg(s) → 2 PO(s) + 3 MgBr2(s)(d) 4 BCI3(g) + 3 SF4(g) ·→ SF,(g) + 2 HF(g) + 4 O2(g)4 BF3(g) + 3 SCI2(t) + 3 Cl2(g)

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Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter3: Equation, The Mole, And Chemical Formulas

Section: Chapter Questions

Problem 3.41QE

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Phosphoric acid is prepared by dissolving phosphorus(V) oxide, P4O10, in water. What is the balanced equation for this reaction? How many grams of P4O10 are required to make 1.19 L of aqueous solution containing 5.50% phosphoric acid by mass? The density of the solution is 1.025 g/mL.
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Write balanced chemical equations for the following reactions. (a) The reaction of aluminum and iron(III) oxide to form iron and aluminum oxide (known as the thermite reaction). (b) The reaction of carbon and water at high temperature to form a mixture of gaseous CO and H2 (known as water gas and once used as a fuel). (c) The reaction of liquid silicon tetrachloride and magnesium forming silicon and magnesium chloride. This is one step in the preparation of ultrapure silicon used in the semiconductor industry

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