Basic Chemistry
6th Edition
ISBN: 9780134878119
Author: Timberlake, Karen C. , William
Publisher: Pearson,
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Chapter 9.3, Problem 11PP
Sodium reacts with oxygen to produce sodium oxide.
a. How many grams of
b. If you have 18.0 g of Na, how many grams of
c. How many grams of
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28
O
6
Chapter 9 Solutions
Basic Chemistry
Ch. 9.1 - Calculate the total mass of the reactants and the...Ch. 9.1 - Calculate the total mass of the reactants and the...Ch. 9.2 - Calculate the total mass of the reactants and the...Ch. 9.2 - Write all of the mole-mole factors for each of the...Ch. 9.2 - For the chemical equations in problem 9.3, write...Ch. 9.2 - For the chemical equations in problem 9.4, write...Ch. 9.2 - The chemical reaction of hydrogen with oxygen...Ch. 9.2 - Ammonia is produced by the chemical reaction of...Ch. 9.2 - Carbon disulfide and carbon monoxide are produced...Ch. 9.2 - In the acetylene torch, acetylene gas burns in...
Ch. 9.3 - Sodium reacts with oxygen to produce sodium oxide....Ch. 9.3 - Nitrogen reacts with hydrogen to produce ammonia....Ch. 9.3 - Ammonia and oxygen react to form nitrogen and...Ch. 9.3 - Iron(III) oxide reacts with carbon to give iron...Ch. 9.3 - Prob. 15PPCh. 9.3 - Calcium cyanamide, CaCN2 , reacts with water to...Ch. 9.3 - Prob. 17PPCh. 9.3 - Prob. 18PPCh. 9.4 - A taxi company has 10 taxis. a. On a certain day,...Ch. 9.4 - Prob. 20PPCh. 9.4 - Prob. 21PPCh. 9.4 - Iron and oxygen react to form iron(III) oxide....Ch. 9.4 - For each of the following reactions, 20.0 g of...Ch. 9.4 - For each of the following reactions, 20.0 g of...Ch. 9.4 - For each of the following reactions, calculate the...Ch. 9.4 - For each of the following reactions, calculate the...Ch. 9.5 - Carbon disulfide is produced by the reaction of...Ch. 9.5 - Iron (III) oxide reacts with carbon monoxide to...Ch. 9.5 - Aluminum reacts with oxygen to produce aluminum...Ch. 9.5 - Propane ( C3H8 ) bums in oxygen to produce carbon...Ch. 9.5 - Prob. 31PPCh. 9.5 - When 56.6 g of calcium is reacted with nitrogen...Ch. 9.6 - In an exothermic reaction, is the energy of the...Ch. 9.6 - In an endothermic reaction, is the energy of the...Ch. 9.6 - Prob. 35PPCh. 9.6 - Prob. 36PPCh. 9.6 - Classify each of the following as exothermic or...Ch. 9.6 - Classify each of the following as exothermic or...Ch. 9.6 - Prob. 39PPCh. 9.6 - a. How many kilojoules are released when 75.0 g of...Ch. 9.6 - Prob. 41PPCh. 9.6 - Calculate the energy change for the reaction...Ch. 9.6 - Prob. 43PPCh. 9.6 - Prob. 44PPCh. 9.6 - In one step in the synthesis of the insecticide...Ch. 9.6 - Another widely used insecticide is carbofuran...Ch. 9 - The chapter sections lo review are shown in...Ch. 9 - The chapter sections lo review are shown in...Ch. 9 - The chapter sections lo review are shown in...Ch. 9 - The chapter sections lo review are shown in...Ch. 9 - The chapter sections lo review are shown in...Ch. 9 - The chapter sections lo review are shown in...Ch. 9 - The chapter sections lo review are shown in...Ch. 9 - The chapter sections lo review are shown in...Ch. 9 - Prob. 55APPCh. 9 - Prob. 56APPCh. 9 - Prob. 57APPCh. 9 - Prob. 58APPCh. 9 - Prob. 59APPCh. 9 - Prob. 60APPCh. 9 - Pentane gas ( C5H12 ) reacts with oxygen to...Ch. 9 - Prob. 62APPCh. 9 - Prob. 63APPCh. 9 - Prob. 64APPCh. 9 - Prob. 65APPCh. 9 - Prob. 66APPCh. 9 - Prob. 67APPCh. 9 - Prob. 68APPCh. 9 - Prob. 69APPCh. 9 - The equation for the reaction of iron and oxygen...Ch. 9 - Prob. 71APPCh. 9 - Prob. 72APPCh. 9 - Prob. 73CPCh. 9 - Prob. 74CPCh. 9 - Prob. 75CPCh. 9 - The following problems are related to the topics...Ch. 9 - Prob. 77CPCh. 9 - Prob. 78CPCh. 9 - Prob. 79CPCh. 9 - Prob. 80CPCh. 9 - The following problems are related to the topics...Ch. 9 - Prob. 82CPCh. 9 - Prob. 83CPCh. 9 - The following problems are related to the topics...Ch. 9 - Prob. 85CPCh. 9 - Prob. 86CP
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- 3. Hydrogen reacts with nitrogen to form ammonia by the following equation: 3 H₂(g) + N2(g) → 2 NH3(g) a. What is the limiting reactant if 1.60 g of hydrogen are mixed with 6.90 g of nitrogen? b. What is the theoretical yield of ammonia (in grams)? c. Calculate the percent yield of ammonia when 7.45 grams of ammonia was experimentally obtained from the reaction? 28 7 /7 > ||| 0 7arrow_forward10.0 grams of methane is burned in an excess of oxygen and the reaction forms 19.8 grams of water in the lab. CH4(g) + 202(g) co2(g) + 2H2O(g)a. What is the percent yield?b. List any reasons why the percentage yield is often less than 100% in a chemical reaction. *arrow_forwardUse the balanced equation, N 2 + O 2------>2 NO, to answer the following questions. a. How many grams of NO are formed from 10.0 g of N 2? b. How many grams of NO are formed from 10.0 g of O 2? c. How many grams of O 2 are needed to react completely with 10.0 g of N 2?arrow_forward
- 3. Hydrogen reacts with nitrogen to form ammonia by the following equation:3 H2(g) + N2(g) → 2 NH3(g)a. What is the limiting reactant if 1.60 g of hydrogen are mixed with 6.90 g of nitrogen?b. What is the theoretical yield of ammonia (in grams)?c. Calculate the percent yield of ammonia when 7.45 grams of ammonia wasexperimentally obtained from the reaction?arrow_forward6. Consider the reaction of solid PbO and gaseous NH₃ to form solid Pb, nitrogen gas, and water vapor. a. The balanced chemical equation is 3 PbO(s) + 2 NH₃(g) → 3 Pb(s) + N₂(g) + 3 H₂O(g). How many moles of NH₃ are required to produce 185.6 grams of Pb based on the balanced chemical equation? b. How many grams of N₂ will be produced from 0.447 moles of PbO balanced chemical equation? c. How many grams of NH₃ will be required to react with 32.7 grams of PbO based on the balanced chemical equation? (Part a shown in picture)arrow_forwardMethyl alcohol (wood alcohol), CH3OH, is produced via the reaction: CO(g) + 2 H2(g ) → CH3OH (I) A. How many grams of methyl alcohol can be produced from 147 g of CO with excess hydrogen present? B. How many grams of methyl alcohol can be produced from 22.1 g of hydrogen with excess CO present? C. How many grams of methyl alcohol can be produced from 147 g of CO and 22.1 g of hydrogen?arrow_forward
- 1. The reaction of iron (III) oxide with carbon monoxide produces iron and carbon dioxide. Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) If you have 39.5g of Fe2O3, how many grams of CO are required for a complete reaction? show your work 2.The reaction of iron (III) oxide with carbon monoxide produces iron and carbon dioxide. Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) How many grams of Fe2O3 are required to produce 4.65g Fe? show your workarrow_forward1. Given the following equation: 2 N2 (g) + 3 H2 (g) →→ 2 NH3 (g) How many grams of H2 are required if 19 grams of N2 reacts? 2. Given the following equation: N2(g)+3H2(g)→2NH3(g)N2(g)+3H2(g)→2NH3(g) How many grams of NH3 are produced if 42.5 grams of N2 and 23.8 grams of H2 react? What is the limiting reactant? N2 H2 NH3 There is no limiting reactantarrow_forwardFes + H209)→ Fez04(s) +H ²(g)| d. If you have 10.0 g of Fe, how many grams of H20 will be needed for a complete reaction?arrow_forward
- 5. Methyl alcohol (CH3OH) is made by reacting carbon monoxide and hydrogen in the presence of certain metal oxide catalysts. What mass of alcohol can be obtained by reacting 40.0 g of CO and 10.0 g of H2? CO (g) + 2 H2 (g) CH3OH (l)arrow_forward5. Consider the following reaction: 3 Hg(OH)2 + 2 H3PO4 Hg3(PO4)2 + 6 H2O How many grams of H3PO4 are needed to produce 10.9 g of Hg3(PO4)2?arrow_forward1.410 pmol CI, x mos,ly I50g SCla= 190.4 g of S,Cl2 Solution that should be followed. Thank youuu This kind of problem is an example of a limiting reactant problem since you are given the quantities of both the reactants and you are asked to calculate for the amount of the product. To solve limiting reactant problems, consider the following steps: Step 1: Write down the known and the unknown quantities in the problem. Given: mass sulfur = 200.0 g mass chlorine= 100 g Unknown: a.) limiting reactant b.) mass of disulfur dichloride (S2Ch) Step 2: Balance the chemical equation. In the problem, the chemical equation is already balanced. Step 3: Convert mass of reactants to moles. Use the molar mass (inverse ) as a conversion factor 100.00 oct, x mol Cl, (8) = 1,410 mol C 70.9 cla 200.0 48.x Imol Sa (R) = 0.7797 mol S, 256.5S Step 4: Calculate the mole ratio of the reactants. To determine the actual ratio of moles, divide the available moles of chlorine by the available moles of sulfur which…arrow_forward
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