46 problems
7 Pages

46 problems

Course Number: CHEM 1310, Fall 2009

College/University: Maryville MO

Word Count: 535

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4.59 Which type of redox reaction leads to the following? (a) An increase in the number of substances (b) A decrease in the number of substances (c) No change in the number of substances 4.60 Why do decomposition reactions typically have compounds as reactants, whereas combination and displacement reactions have one or more elements? 4.61 Which of the three types of reactions discussed in this section commonly...

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Which 4.59 type of redox reaction leads to the following? (a) An increase in the number of substances (b) A decrease in the number of substances (c) No change in the number of substances 4.60 Why do decomposition reactions typically have compounds as reactants, whereas combination and displacement reactions have one or more elements? 4.61 Which of the three types of reactions discussed in this section commonly produce one or more compounds? 4.62 Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction: (a) Sb(s) + Cl 2(g) SbCl 3(s) (b) AsH 3(g) As(s) + H 2(g) (c) Mn(s) + Fe(NO 3)3(aq) Mn(NO 3)2(aq) + Fe(s) 4.63 Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction: (a) Mg(s) + H 2O(g) Mg(OH) 2(s) + H 2(g) (b) Cr(NO 3)3(aq) + Al(s) Al(NO 3)3(aq) + Cr(s) (c) PF 3(g) + F 2(g) PF 5(g) 4.64 Predict the product(s) and write a balanced equation for each of the following redox reactions: (a) N 2(g) + H 2(g) (c) Ba(s) + H 2O(l ) 4.65 Predict the product(s) and write a balanced equation for each of the following redox reactions: (a) Fe(s) + HClO 4(aq) (b) S8(s) + O2(g) 4.66 Predict the product(s) and write a balanced equation for each of the following redox reactions: (a) Cesium + iodine (b) Aluminum + aqueous manganese(II) sulfate (c) Sulfur dioxide + oxygen (d) Propane and oxygen (e) Write a balanced net ionic equation for (b). 4.67 Predict the product(s) and write a balanced equation for each of the following redox reactions: (a) Pentane 12) (C5H + oxygen (b) Phosphorus trichloride + chlorine (c) Zinc + hydrobromic acid (d) Aqueous potassium iodide + bromine (e) Write a balanced net ionic equat ion for (d). 4.68 How m any grams of O2 can be prepared from the thermal decomposition of 4.27 kg of HgO? Name and calculate the mass (in kg) of the other product. 4.69 How many grams of chlorine gas can be produced from the electrolytic decomposition of 874 g of calcium chloride? Name and calculate the mass (in g) of the other product. 4.70 In a combination reaction, 1.62 g of lithium is mixed with 6.00 g of oxygen. (a) Which reactant is present in excess? (b) How many moles of product are formed? (c) After react ion, how m any grams of each reactant and product are present? 4.71 In a combination reaction, 2.22 g of magnesium is heated with 3.75 g of nitrogen. (a) Which reactant is present in excess? (b) How many moles of product are formed? (c) After reaction, how many grams of each reactant and product are present? 4.72 A m ixt ure of CaCO3 and CaO weighing 0.693 g was heated to produce gaseous CO2. After heating, the remaining solid weighed 0.508 g. Assuming all the CaCO3 broke down to CaO and CO2, calculate the mass percent of CaCO3 in the original mixture. 4.73 Before arc welding was developed, a displacement reaction involving aluminum and iron(III) oxide was commonly used to produce molten iron (the thermite process). This reaction was used, for example, to connect sections of iron railroad track. Calculate the mass of molten iron produced when 1.00 kg of aluminum reacts with 2.00 mol of iron(III) oxide.
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