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introductory chemistry concepts

Introductory Chemistry Concepts And Critical Thinking 7th Edition Charles Corwin - Solutions

Calculate the mass of potassium iodide (166.00 g/mol) required to yield 1.78 g of mercury(II) iodide precipitate (454.39 g/mol): 2 KI(s) + Hg(NO3)2(ag) Hgl₂(s) + 2 KNO3(aq)
In general, how many unit factors are required to solve a mass–mass stoichiometry problem?
Illustrate the conservation of mass law using the molar masses of reactants and products for each substance in the following balanced equations.(a) 2 N2(s) + 3 O2(g) → 2 N2O3(s)(b) 2 N2(s) + 5 O2(g) → 2 N2O5(s).
Calculate the volume of hydrogen gas produced at STP from 1.55 g of sodium metal in water, given the unbalanced equation for the reaction: Na(s) + H₂O(1) NaOH(aq) + H₂(g)
What STP volume of hydrogen gas is produced from decomposing 5.00 g of water (18.02 g/mol)? 2 H2O(l) → 2 H2(g) + O2(g)(a) 1.55 L(b) 3.11 L(c) 5.00 L(d) 6.22 L(e) 12.4 L.
In an automobile collision, sodium azide, NaN3, decomposes and fills an air bag with nitrogen gas. If an air bag contains 100.0 g of NaN3(65.02 g/mol), what is the volume of nitrogen gas produced at STP? The equation for the reaction is 2 NaN3(s) spark 2 Na(s) + 3 N₂(8)
What are the three steps in the unit analysis method of problem solving?
Illustrate the conservation of mass law using the molar masses of reactants and products for each substance in the following balanced equations.(a) P4(s) + 3 O2(g) → 2 P2O3(s)(b) P4(s) + 5 O2(g) → 2 P2O5(s).
Calculate the mass of aluminum metal required to release 2160 mL of hydrogen gas at STP from sulfuric acid given the unbalanced equation for the reaction: Al(s) + H₂SO4(aq) Al2(SO4)3(aq) + H₂(8)
What volume of oxygen gas is released from decomposing water if 5.00 mL of hydrogen gas is produced (assume constant temperature and pressure)? 2 H2O(l) → 2 H2(g) + O2(g) (a) 2.50 mL(b) 5.00 mL(c) 7.50 mL(d) 10.0 mL(e) 20.0 mL.
Baking soda can be used as a fire extinguisher. When heated, it decomposes to carbon dioxide gas, which can smother a fire. If a sample of NaHCO3 (84.01 g/mol) produces 0.500 L of carbon dioxide gas at STP, what is the mass of the sample? 2 NaHCO3(s) Na₂CO3(s) + H₂O(g) + CO₂(g)
In general, how many unit factors are required to solve a mass–volume stoichiometry problem?
Given the following decomposition reaction, calculate the moles of oxygen gas produced from 5.00 mol of H2O2. 2 H₂O₂(1) 2 H₂O(l) + O₂(g)
Calculate the volumes of(a) Hydrogen chloride gas and(b) Oxygen gas that react to yield 40.00 mL of chlorine gas given the following unbalanced equation. Assume that all gases are at the same temperature and pressure. HCl(g) + O₂(g) 02(8) Cl₂(g) + H₂O(g)
Consider the limiting reactant concept and predict how many moles of steam are released from the reaction of 5.00 mol of hydrogen gas and 5.00 mol of oxygen gas (assume constant temperature and pressure)? 2 H2(g) + O2(g) → 2 H2O(g) (a) 2.50 mol(b) 5.00 mol(c) 10.0 mol(d) 15.0
In general, how many unit factors are required to solve a volume–volume stoichiometry problem?
In the Haber process, nitrogen and hydrogen gases combine to give ammonia gas. If 5.55 L of nitrogen gas is available, calculate the volume of ammonia that is produced. Assume that all volumes of gas are measured under constant conditions of 500 °C and 300 atm pressure: N + Η Η + N2(g) + 3
Given the following decomposition reaction, calculate the moles of water produced from 5.00 mol of H2O2. 2 H₂O₂(1) 2 H₂O(1) + O₂(g)
Calculate the volumes of(a) Nitrogen monoxide gas(b) Oxygen gas that react to yield 50.0 mL of nitrogen dioxide gas given the following unbalanced equation. Assume all gases are at the same temperature and pressure. NO(g) + 0₂(8) ↑ NO₂(g)
Consider the limiting reactant concept and predict how many liters of steam are released from the reaction of 5.00 L of hydrogen gas and 5.00 L of oxygen gas (assume constant temperature and pressure)? 2 H2(g) + O2(g) → 2 H2O(g) (a) 2.50 L(b) 5.00 L(c) 10.0 L(d) 15.0 L(e) None of the
In the Ostwald process, ammonia and oxygen gases combine to give nitrogen monoxide gas and steam using a platinum catalyst. The NO is then converted to nitric acid, HNO3. If 50.0 L of NO are produced, what is the volume of NH3 required? Assume all gaseous volumes are measured at the same conditions
Given the following decomposition reaction, calculate the moles of oxygen gas produced from 5.00 mol of LiClO3. 2 LiClO3(s) 2 LiCl(s) + O₂(g)
Why is only one unit factor usually required to solve a volume–volume stoichiometry problem?
The decomposition of 5.00 g of water releases 4.00 g of oxygen gas. If the calculated mass of oxygen is 4.44 g, what is the percent yield? 2 H2O(l) → 2 H2(g) + O2(g)(a) 80.0%(b) 88.8%(c) 90.1%(d) 111%(e) 125%.
A 1.00 mol sample of iron(II) oxide is heated with 1.00 mol of aluminum metal and converted to molten iron. Identify the limiting reactant, and calculate the moles of iron produced in the so-called Thermite reaction: 3 FeO (1) + 2 Al(1) 3 Fe(l) + Al₂O3(s)
Given the following decomposition reaction, calculate the moles of lithium chloride produced from 5.00 mol of LiClO3. 2 LiClO3(s) 2 LiCl(s) + O₂(8)
A Tour de France cyclist has 10 tires and 3 frames. How many complete bicycles can be assembled?
In a reaction, 75.0 g of manganese(IV) oxide react with 30.0 g of aluminum. Identify the limiting reactant and calculate the mass of aluminum oxide produced: 3 MnO₂(1) + 4 Al(1) 3 Mn(1) + 2 Al₂O3(s)
What is required before applying unit analysis to solve a stoichiometry problem?
Indicate the limiting reactant shown in the following illustration: ZnS(s) S (s)suz (s)S + (s)uz
How many moles of chlorine gas react with 0.100 mol of metallic iron given the unbalanced chemical equation? How many moles of iron(III) chloride are produced? Fe(s) + Cl₂(g) FeCl3(s)
In a reaction, 50.0 g of manganese(IV) oxide reacts with 25.0 g of aluminum. Identify the limiting reactant and calculate the mass of manganese metal produced. The equation for the reaction is 3 MnO₂(1) + 4 Al(1) 3 Mn(1) + 2 Al2O3(s)
How many unit factors are typically required to solve a mass–mass problem?
Ethane undergoes combustion to give carbon dioxide and water. If 10.0 L of C2H6 reacts with 25.0 L of O2, what is the limiting reactant? Assuming constant conditions, what is the volume of CO2 produced? The equation is 2 C₂H6(g) + 7 0₂(8) spark 4 CO₂(g) + 6 H₂O(g)
Indicate the limiting reactant shown in the following illustration: Zn(s) + S(s) ZnS(s)
How many moles of barium metal react to produce 0.100 mol of barium nitride given the unbalanced chemical equation? How many moles of nitrogen gas react? Ba(s) + N₂(g) Ba3N₂(s)
In oxyacetylene welding, acetylene reacts with oxygen to give carbon dioxide and water. If 25.0 mL of C2H2 reacts with 75.0 mL of O2, what is the limiting reactant? Assuming constant conditions, what is the volume of CO2 produced? 2 C₂H₂(g) +50₂(8) spark 4 CO₂(g) + 2 H₂O(g)
How many unit factors are typically required to solve a mass–volume problem?
Ammonium nitrate is used in explosives and is produced by the reaction of ammonia, NH3, and nitric acid. The equation for the reaction isIf 15.0 kg of ammonia gives an actual yield of 65.3 kg of ammonium nitrate, what is the percent yield? The calculated yield of ammonium nitrate for the experiment
Is it possible to have a percent yield greater than 100%?
How many moles of propane gas, C3H8, react with 2.50 mol of oxygen gas given the unbalanced chemical equation? How many moles of carbon dioxide are produced? C3H8(g) + O₂(g) CO₂(g) + H₂O(g)
How many unit factors are typically required to solve a volume–volume problem?
A student dissolves 1.50 g of copper(II) nitrate in water. After adding aqueous sodium carbonate solution, the student obtains 0.875 g of CuCO3 precipitate. If the theoretical yield is 0.988 g, what is the percent yield? Cu(NO3)2(aq) + Na₂CO3(aq) CuCO3(s) + 2 NaNO3(aq)
How many moles of butane gas, C4H10, react to produce 2.50 mol of water given the unbalanced chemical equation? How many moles of oxygen gas react? (8)0³H+ (8)²00 (8)²0 + (8⁰¹H¹)
Gasoline and air undergo a combustion reaction in an automobile engine. What is the limiting reactant? What is the excess reactant?
Silver metal heated with yellow sulfur powder gives Ag2S.Complete the following illustrations by drawing the product and excess reactant. Indicate the element that is the limiting reactant in each example. A 2 Ag(s) + S(s) Ag₂S(s)
Classify the following type of stoichiometry problem: How many grams of carbon dioxide gas are produced from the decomposition of 1.10 g NaHCO3?
Classify the following type of stoichiometry problem: How many grams of baking soda decompose to give 1.25 g Na2CO3?
Classify the following type of stoichiometry problem: How many grams of ferric oxide are produced from iron metal and 50.0 L of steam?
Classify the following type of stoichiometry problem: How many liters of steam react with iron metal to yield 1.88 g FeO?
What is the mass of mercury that can be prepared from 1.25 g of cobalt metal? Co(s) + HgCl₂(aq) CoCl3(aq) + Hg(1)
Classify the following type of stoichiometry problem: How many milliliters of hydrogen chloride gas are produced from hydrogen and 25.0 mL Cl2?
What is the mass of zinc oxide that can be prepared from 1.00 g of zinc metal? 2 Zn(s) + O₂(g) 2 ZnO(s)
Classify the following type of stoichiometry problem: How many milliliters of chlorine gas react with 50.0 mL H2?
How many grams of oxygen gas react to give 1.50 g of ZnO according to the equation in Exercise 21?Exercise 21What is the mass of zinc oxide that can be prepared from 1.00 g of zinc metal? 2 Zn(s) + O₂(g) →→→ 2 ZnO(s)
What is the mass of product that can be prepared from 3.45 g of bismuth metal. 2 Bi(s) + 3Cl₂(g) 2 BiCl3(s)
How many grams of chlorine gas react to give 3.52 g of BiCl3 according to the equation in Exercise 23?Exercise 23What is the mass of product that can be prepared from 3.45 g of bismuth metal. 2 Bi(s) + 3Cl₂(g) 2 BiCl3(s)
What is the mass of silver that can be prepared from 1.25 g of copper metal? Cu(s) + 2 AgNO3(aq) - Cu(NO3)2(aq) + 2 Ag(s)
How many grams of copper react to give 1.50 g Ag according to the equation in Exercise 25?Exercise 25 What is the mass of silver that can be prepared from 1.25 g of copper metal? Cu(s) + 2 AgNO3(aq) - Cu(NO3)2(aq) + 2 Ag(s)
How many grams of mercuric chloride react to give 5.11 g of Hg according to the equation in Exercise 27?Exercise 27What is the mass of mercury that can be prepared from 1.25 g of cobalt metal? Co(s) + HgCl₂(aq) CoCl3(aq) + Hg(1)
What is the mass of calcium phosphate that can be prepared from 1.78 g Na3PO4? Na3PO4(aq) + Ca(OH)₂(aq) Ca3(PO4)2(s) + NaOH(aq)
How many milliliters of carbon dioxide gas at STP are produced from the decomposition of 1.75 g of sodium hydrogen carbonate? 2 NaHCO3(s)→→→ Na₂CO3(s) Na₂CO3(s) + H2₂O(l) + CO₂(g)
How many grams of sodium hydrogen carbonate decompose to give 25.0 mL of carbon dioxide gas at STP according to the equation in Exercise 31?Exercise 31How many milliliters of carbon dioxide gas at STP are produced from the decomposition of 1.75 g of sodium hydrogen carbonate? 2 NaHCO3(s)→→→
How many grams of calcium hydroxide react to give 2.39 g of Ca3(PO4)2 according to the equation in Exercise 29?Exercise 29What is the mass of calcium phosphate that can be prepared from 1.78 g Na3PO4?
How many milliliters of carbon dioxide gas at STP are produced from the decomposition of 5.00 g of iron(III) carbonate? Fe₂(CO3)3(S) Fe₂O3(s) + 3CO₂(8)
How many grams of iron(III) carbonate decompose to give 50.0 mL of carbon dioxide gas at STP according to the equation in Exercise 33?Exercise 33How many milliliters of carbon dioxide gas at STP are produced from the decomposition of 5.00 g of iron(III) carbonate? Fe₂(CO3)3(S) Fe₂O3(s) +
How many milliliters of oxygen gas at STP are produced from the decomposition of 1.55 g of hydrogen peroxide, H2O2? HO(1) ه H2O(1) + O2(g)
How many grams of mercury(II) oxide decompose to give 50.0 mL of oxygen gas at STP according to the equation in Exercise 35?Exercise 35How many milliliters of oxygen gas at STP are released from the decomposition of 2.50 g of mercury(II) oxide? 2 HgO(s) 2 Hg(1) + O₂(8)
How many milliliters of oxygen gas at STP are released from the decomposition of 2.50 g of mercury(II) oxide? 2 HgO(s) 2 Hg(1) + O₂(8)
Assuming the same temperature and pressure for each gas, how many milliliters of oxygen gas react with 10.0 mL of carbon monoxide? O₂(g) →→→2 CO₂(g) 2 CO(g) + O2(g)
How many grams of hydrogen peroxide decompose to give 50.0 mL of oxygen gas at STP according to the equation in Exercise 37?Exercise 37How many milliliters of oxygen gas at STP are produced from the decomposition of 1.55 g of hydrogen peroxide, H2O2? HO(1) ه H2O(1) + O2(g)
Assuming the same temperature and pressure for each gas, how many liters of nitrogen gas react with 50.0 L of hydrogen gas? 3 H₂(g) + N₂(g) 2 NH3(8)
Assuming the same temperature and pressure for each gas, how many liters of ammonia are produced from 50.0 L of H2 according to the equation in Exercise 39?Exercise 39Assuming the same temperature and pressure for each gas, how many liters of nitrogen gas react with 50.0 L of hydrogen gas? 3
Assuming the same temperature and pressure for each gas, how many milliliters of carbon dioxide are produced from 10.0 mL of CO according to the equation in Exercise 41?Exercise 41Assuming the same temperature and pressure for each gas, how many milliliters of oxygen gas react with 10.0 mL of
Assuming constant conditions, how many milliliters of chlorine gas react to yield 1.75 L of dichlorine trioxide? Cl₂(g) + O₂(g) Cl₂O3(g)
Assuming constant conditions, how many milliliters of oxygen gas react to give 1.75 L of Cl2O3 according to the equation in Exercise 43?Exercise 43 Assuming constant conditions, how many milliliters of chlorine gas react to yield 1.75 L of dichlorine trioxide? Cl₂(g) + O₂(g) Cl₂O3(g)
Assuming constant conditions, what volume of sulfur trioxide gas is produced from 25.0 L of oxygen gas? SO₂(g) + O₂(g) SO3(g)
Assuming constant conditions, what volume of sulfur dioxide gas reacts with 25.0 L of O2 according to the equation in Exercise 45?Exercise 45Assuming constant conditions, what volume of sulfur trioxide gas is produced from 25.0 L of oxygen gas? SO₂(g) + O₂(g) SO3(g)
Assuming constant conditions, what volume of nitrogen gas reacts to yield 500.0 cm3 of dinitrogen pentaoxide? (8)O°N < (8)O+ (8) N
If 1.50 mol of nitrogen monoxide gas and 1.50 mol of oxygen gas react, what is the limiting reactant and how many moles of NO2 are produced from the reaction? 2 NO(g) + O₂(8) 2 NO₂(g)
Assuming constant conditions, what volume of oxygen gas reacts to yield 500.0 cm3 of N2O5 according to the equation in Exercise 47?Exercise 47Assuming constant conditions, what volume of nitrogen gas reacts to yield 500.0 cm3 of dinitrogen pentaoxide? (8)O°N < (8)O+ (8) N
If 5.00 mol of nitrogen gas and 5.00 mol of oxygen gas react, what is the limiting reactant and how many moles of NO are produced from the reaction? N₂(g) + O₂(g) 2 NO(g)
If 0.125 mol of nitrogen gas and 0.125 mol of oxygen gas react, what is the limiting reactant and how many moles of NO are produced according to the equation in Exercise 49?Exercise 49If 5.00 mol of nitrogen gas and 5.00 mol of oxygen gas react, what is the limiting reactant and how many moles of
If 1.50 mol of nitrogen monoxide gas and 2.50 mol of oxygen gas react, what is the limiting reactant and how many moles of NO2 are produced according to the equation in Exercise 51?Exercise 51If 1.50 mol of nitrogen monoxide gas and 1.50 mol of oxygen gas react, what is the limiting reactant and
If 5.00 mol of hydrogen gas and 5.00 mol of oxygen gas react, what is the limiting reactant and how many moles of water are produced from the reaction? 2 H₂(g) + O2(g) 2 H₂O(1)
If 5.00 mol of hydrogen gas and 1.50 mol of oxygen gas react, what is the limiting reactant and how many moles of water are produced according to the equation in Exercise 53?Exercise 53If 5.00 mol of hydrogen gas and 5.00 mol of oxygen gas react, what is the limiting reactant and how many moles of
If 1.00 mol of ethane gas and 5.00 mol of oxygen gas react, what is the limiting reactant and how many moles of water are produced from the reaction? 2C,H%(g) +7O2(g) → 4 CO2(g) +6H,O(g)
If 1.00 mol of ethane gas and 3.00 mol of oxygen gas react, what is the limiting reactant and how many moles of water are produced according to the equation in Exercise 55?Exercise 55If 1.00 mol of ethane gas and 5.00 mol of oxygen gas react, what is the limiting reactant and how many moles of
The following table indicates the amounts of Co and S before reaction. Complete the table after reactions (a) and (b) according to the balanced equation: Co(s) + S(s) A, CoS(s)
The following table indicates the amounts of Co and S before reaction. Complete the table after reactions (a) and (b) according to the balanced equation: 2 Co(s) + 3 S(s) C0₂S3(s)
If 50.0 g of molten iron(II) oxide reacts with 10.0 g of magnesium, what is the mass of iron produced? FeO (1) + Mg(1) Fe(l) + MgO(s)
If 0.605 g of magnesium hydroxide reacts with 1.00 g of sulfuric acid, what is the mass of magnesium sulfate produced according to the equation in Exercise 63?Exercise 63If 1.00 g of magnesium hydroxide reacts with 0.605 g of sulfuric acid, what is the mass of magnesium sulfate produced?
If 50.0 g of molten iron(II) oxide reacts with of 20.0 g magnesium, what is the mass of iron produced according to the equation in Exercise 59?Exercise 59If 50.0 g of molten iron(II) oxide reacts with 10.0 g of magnesium, what is the mass of iron produced? FeO (1) + Mg(1) Fe(l) + MgO(s)
If 50.0 g of molten iron(III) oxide reacts with 15.0 g of aluminum, what is the mass of iron produced? Fe₂O3(1) + Al(1) Fe(l) + Al₂O3(s)
If 50.0 g of molten iron(III) oxide reacts with 25.0 g of aluminum, what is the mass of iron produced according to the equation in Exercise 61?Exercise 61If 50.0 g of molten iron(III) oxide reacts with 15.0 g of aluminum, what is the mass of iron produced? Fe₂O3(1) + Al(1) Fe(l) + Al₂O3(s)
If 1.00 g of magnesium hydroxide reacts with 0.605 g of sulfuric acid, what is the mass of magnesium sulfate produced? Mg(OH)₂(s) + H₂SO4(1)→ MgSO4(s) + H₂O(1)
If 1.00 g of aluminum hydroxide reacts with 3.00 g of sulfuric acid, what is the mass of water produced? Al(OH)3(s) + H₂SO4(1) Al₂(SO4)3(aq) + H₂O(1)
If 3.00 g of aluminum hydroxide reacts with 1.00 g of sulfuric acid, what is the mass of water produced according to the equation in Exercise 65?Exercise 65If 1.00 g of aluminum hydroxide reacts with 3.00 g of sulfuric acid, what is the mass of water produced? Al(OH)3(s) +
If 45.0 mL of nitrogen gas reacts with 95.0 mL of oxygen gas, what is the volume of NO2 produced? Assume all gases are at the same temperature and pressure. N₂(g) + O₂(g) NO₂(g)
If 95.0 mL of nitrogen gas reacts with 45.0 mL of oxygen gas, what is the volume of NO2 produced according to the equation in Exercise 67? Assume all gases are at the same temperature and pressure.Exercise 67If 45.0 mL of nitrogen gas reacts with 95.0 mL of oxygen gas, what is the volume of NO2

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