Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Textbook Question
Chapter 5, Problem 100IL
On a cold day, you can warm your hands with a “heat pad,” a device that uses the oxidation of iron to produce energy as heat.
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)
A hand warmer uses the oxidation of iron as a source of thermal energy.
What mass of iron is needed to supply the energy required to warm 15 mL of water (d = 1.00 g/mL) from 23 °C to 37 °C?
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5. Calculate the total amount of heat transferred as 50 g of wat Specific heat H₂O (g) 2.00 J/g°C
-10 °C.
Specific heat H₂O (1)
Specific heat H₂O (s)
4.18 J/g°C
2.11 J/g°C
Heat of vaporization
2260 J/g
Heat of fusion
334 J/g
Melting point
0°C
6. Calculate the total amount of heat transferred as 25 g of
water is heated from 50 °C to 100 °C as a gas.
Boiling point
100 °C
Calculate the total amount of heat
transferred as 50 g of Water -10°C.
Calculate the total amount of heat
transferred as 25 g of water is heated
from 50°C to 100°C as a gas.
\table[[Specific heat H₂O(g), 2.00°C
Η
2
g
5. Calculate the total amount of heat transferred as 50 g of wat Specific heat H₂O (g) 2.00 J/g°C
-10 °C.
4.18 J/g°C
2.11 J/g°C
2260 J/g
334 J/g
Specific heat H₂O (1)
Specific heat H₂O (s)
Heat of vaporization
Heat of fusion
Melting point
6. Calculate the total amount of heat transferred as 25 g of
water is heated from 50 °C to 100 °C as a gas.
Boiling point
100 °C
0°C
Write formulas for ionic compounds composed of the following ions.
Use units as a guide to your solutions.
24. sodium and nitrate
25. calcium and chlorate
26. aluminum and carbonate
27.
CHALLENGE Write the formula for an ionic compound formed by ions from a group 2 element and polyatomic ions composed of only carbon and oxygen.show work step by step
Chapter 5 Solutions
Chemistry & Chemical Reactivity
Ch. 5.1 - 1. Which of the following processes is...Ch. 5.1 - 2. Your skin cools as perspiration evaporates. Is...Ch. 5.2 - You did an experiment in which you found that 59.8...Ch. 5.2 - A 15.5-g piece of chromium, heated to 100.0 C, is...Ch. 5.2 - Prob. 1RCCh. 5.2 - Prob. 2RCCh. 5.3 - Calculate the amount of energy necessary to raise...Ch. 5.3 - To make a glass of iced tea, you pour 250 mL of...Ch. 5.3 - 1. Which of the following processes requires the...Ch. 5.3 - Ice (5.0 g) at 0 C is added to 25 g of liquid...
Ch. 5.4 - Nitrogen gas (2.75 L) is confined in a cylinder...Ch. 5.4 - Which of the following processes will lead to a...Ch. 5.4 - 2. In which of the following reactions is there a...Ch. 5.5 - The combustion of ethane, C2H6, has an enthalpy...Ch. 5.5 - 1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s),...Ch. 5.5 - 2. For the reaction 2 CO(g) + O2(g) → 2 CO2(g)....Ch. 5.6 - Assume 200. mL of 0.400 M HCl is mixed with 200....Ch. 5.6 - A 1.00-g sample of ordinary table sugar (sucrose,...Ch. 5.6 - A student used a coffee-cup calorimeter to...Ch. 5.6 - If, in the experiment described in the previous...Ch. 5.7 - Use Hesss law to calculate the enthalpy change for...Ch. 5.7 - Calculate the standard enthalpy of combustion for...Ch. 5.7 - Prob. 1RCCh. 5.7 - The standard enthalpies of formation of KNO3(s)...Ch. 5.7 - Prob. 2QCh. 5.7 - The decomposition of nitroglycerin (C3H5N3O9)...Ch. 5.7 - Prob. 2RCCh. 5 - Define the terms system and surroundings. What...Ch. 5 - What determines the directionality of energy...Ch. 5 - Identify whether the following processes are...Ch. 5 - Identify whether the following processes are...Ch. 5 - The molar heat capacity of mercury is 28.1 J/mol ...Ch. 5 - The specific heat capacity of benzene (C6H6) is...Ch. 5 - The specific heat capacity of copper metal is...Ch. 5 - How much energy as heat is required to raise the...Ch. 5 - The initial temperature of a 344-g sample of iron...Ch. 5 - After absorbing 1.850 kJ of energy as heat, the...Ch. 5 - A 45.5-g sample of copper at 99.8 C is dropped...Ch. 5 - One beaker contains 156 g of water at 22 C, and a...Ch. 5 - A 182-g sample of gold at some temperature was...Ch. 5 - When 108 g of water at a temperature of 22.5 C is...Ch. 5 - A 13.8-g piece of zinc is heated to 98.8 C in...Ch. 5 - A 237-g piece of molybdenum, initially at 100.0 C,...Ch. 5 - How much energy is evolved as heat when 1.0 L of...Ch. 5 - The energy required to melt 1.00 g of ice at 0 C...Ch. 5 - How much energy is required to vaporize 125 g of...Ch. 5 - Chloromethane, CH3CI, arises from microbial...Ch. 5 - The freezing point of mercury is 38.8 C. What...Ch. 5 - What quantity of energy, in joules, is required to...Ch. 5 - Ethanol, C2HsOH, boils at 78.29 C. How much...Ch. 5 - A 25.0-mL sample of benzene at 19.9 C was cooled...Ch. 5 - As a gas cools, it is compressed from 2.50 L to...Ch. 5 - A balloon expands from 0.75 L to 1.20 L as it is...Ch. 5 - A balloon does 324 J of work on the surroundings...Ch. 5 - As the gas trapped in a cylinder with a movable...Ch. 5 - When 745 J of energy in the form of heat is...Ch. 5 - The internal energy of a gas decreases by 1.65 kJ...Ch. 5 - A volume of 1.50 L of argon gas is confined in a...Ch. 5 - Nitrogen gas is confined in a cylinder with a...Ch. 5 - Nitrogen monoxide, a gas recently found to be...Ch. 5 - Calcium carbide, CaC2, is manufactured by the...Ch. 5 - Isooctane (2,2,4-trimethylpentane), one of the...Ch. 5 - Acetic acid. CH3CO2H, is made industrially by the...Ch. 5 - You mix 125 mL of 0.250 M CsOH with 50.0 mL of...Ch. 5 - You mix 125 mL of 0.250 M CsOH with 50.0 mL of...Ch. 5 - A piece of titanium metal with a mass of 20.8 g is...Ch. 5 - A piece of chromium metal with a mass of 24.26 g...Ch. 5 - Adding 5.44 g of NH4NO3(s) to 150.0 g of water in...Ch. 5 - You should use care when dissolving H2SO4 in water...Ch. 5 - Sulfur (2.56 g) was burned in a constant-volume...Ch. 5 - Suppose you burned 0.300 g of C(s) in an excess of...Ch. 5 - Suppose you burned 1.500 g of benzoic acid,...Ch. 5 - A 0.692-g sample of glucose, C6H12O6, was burned...Ch. 5 - An ice calorimeter can be used to determine the...Ch. 5 - A 9.36-g piece of platinum was heated to 98.6 C in...Ch. 5 - The enthalpy changes for the following reactions...Ch. 5 - The enthalpy changes of the following reactions...Ch. 5 - Enthalpy changes for the following reactions can...Ch. 5 - You wish to know the enthalpy change for the...Ch. 5 - Write a balanced chemical equation for the...Ch. 5 - Write a balanced chemical equation for the...Ch. 5 - (a) Write a balanced chemical equation for the...Ch. 5 - (a) Write a balanced chemical equation for the...Ch. 5 - Use standard enthalpies of formation in Appendix L...Ch. 5 - Use standard enthalpies of formation in Appendix L...Ch. 5 - The first step in the production of nitric acid...Ch. 5 - The Romans used calcium oxide, CaO, to produce a...Ch. 5 - The standard enthalpy of formation of solid barium...Ch. 5 - An important step in the production of sulfuric...Ch. 5 - The enthalpy change for the oxidation of...Ch. 5 - The enthalpy change for the oxidation of styrene....Ch. 5 - Prob. 65GQCh. 5 - Prob. 66GQCh. 5 - For each of the following, define a system and its...Ch. 5 - Prob. 68GQCh. 5 - Use Appendix L to find the standard enthalpies of...Ch. 5 - You have a large balloon containing 1.0 mol of...Ch. 5 - Determine whether energy as heat is evolved or...Ch. 5 - Determine whether energy as heat is evolved or...Ch. 5 - Use standard enthalpies of formation to calculate...Ch. 5 - Which evolves more energy on cooling from 50 C to...Ch. 5 - You determine that 187 J of energy as heat is...Ch. 5 - Calculate the quantity of energy required to...Ch. 5 - You add 100.0 g of water at 60.0 C to 100.0 g of...Ch. 5 - Three 45-g ice cubes at 0 C are dropped into 5.00 ...Ch. 5 - Suppose that only two 45-g ice cubes had been...Ch. 5 - You take a diet cola from the refrigerator and...Ch. 5 - The standard molar enthalpy of formation of...Ch. 5 - Chloromethane, CH3Cl, a compound found throughout...Ch. 5 - Prob. 83GQCh. 5 - Camping stoves are fueled by propane (C3H8),...Ch. 5 - Prob. 85GQCh. 5 - Prob. 86GQCh. 5 - (a) Calculate the enthalpy change, rH, for the...Ch. 5 - You drink 350 mL of diet soda that is at a...Ch. 5 - Chloroform, CHCl3, is formed from methane and...Ch. 5 - Water gas, a mixture of carbon monoxide and...Ch. 5 - Using standard enthalpies of formation, verify...Ch. 5 - A piece of lead with a mass of 27.3 g was heated...Ch. 5 - A 192-g piece of copper is heated to 100.0 C in a...Ch. 5 - Insoluble AgCl(s) precipitates when solutions of...Ch. 5 - Insoluble PbBr2(s) precipitates when solutions of...Ch. 5 - The value of U for the decomposition of 7.647 g of...Ch. 5 - A bomb calorimetric experiment was run to...Ch. 5 - The meals-ready-to-eat (MREs) in the military can...Ch. 5 - On a cold day, you can warm your hands with a heat...Ch. 5 - Without doing calculations, decide whether each of...Ch. 5 - Prob. 102SCQCh. 5 - You want to determine the value for the enthalpy...Ch. 5 - Prepare a graph of specific heat capacities for...Ch. 5 - Prob. 105SCQCh. 5 - You are attending summer school and living in a...Ch. 5 - Prob. 107SCQCh. 5 - Prob. 108SCQCh. 5 - Prob. 109SCQCh. 5 - Peanuts and peanut oil are organic materials and...Ch. 5 - Isomers are molecules with the same elemental...Ch. 5 - Prob. 112SCQCh. 5 - Prob. 113SCQCh. 5 - A piece of gold (10.0 g, CAu = 0.129 J/g K) is...Ch. 5 - Methane, CH4, can be converted to methanol, which,...Ch. 5 - Calculate rH for the reaction 2 C(s) + 3 H2(g) + ...Ch. 5 - You have the six pieces of metal listed below,...Ch. 5 - Sublimation of 1.0 g of dry ice. CO2(s), forms...Ch. 5 - In the reaction of two moles of gaseous hydrogen...
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- ADDITIONAL PRACTICE PRACTICE Problems Write formulas for ionic compounds composed of the following ions. Use units as a guide to your solutions. 24. sodium and nitrate 25. calcium and chlorate 26. aluminum and carbonate 27. CHALLENGE Write the formula for an ionic compound formed by ions from a group 2 element and polyatomic ions composed of only carbon and oxygen. ounds 1998arrow_forward7:35 < Dji Question 19 of 22 5G 50% Submit What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 × 10-9) and 0.120 mol of KBRO in 2.0 L of solution? | 1 2 3 ☑ 4 5 6 C 7 8 ☐ 9 +/- Tap here for additional resources ||| 0 ×10 Гarrow_forwardaw the major substitution products you would expect for the reaction shown below. If substitution would not occur at a significant rate under these conditions, check the box underneath the drawing area instead. Be sure you use wedge and dash bonds where necessary, for example to distinguish between major products. Note for advanced students: you can assume that the reaction mixture is heated mildly, somewhat above room temperature, but strong heat or reflux is not used. B C Br HO O Substitution will not occur at a significant rate. Explanation Check + Х Click and drag to start drawing a structure. © 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibarrow_forward
- Complete the following reactions with the necessary reagents to complete the shown transformation. Example: 1. 2. ? 3. 018 Br OH Answer: H₂O, H2SO4, HgSO4arrow_forward7:34 • < Question 18 of 22 5G 50% Submit What is the pH of a buffer made from 0.220 mol of HCNO (Ka = 3.5 × 10-4) and 0.410 mol of NaCNO in 2.0 L of solution? 1 2 3 ☑ 4 5 6 C 7 8 | 9 +/- 0 ×10 Tap here for additional resources ||| Гarrow_forward6:46 ✔ 5G 58% < Question 7 of 22 Submit What is the primary species in solution at the halfway point in a titration of NH3 with HBr? A NH3 and H+ B NH₁+ and H+ C NH4+ D NH3 and NH4+ Tap here for additional resources |||arrow_forward
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