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chemistry principles and practice

Chemistry Principles And Practice 3rd Edition Daniel L. Reger, Scott R. Goode, David W. Ball - Solutions

To lose weight, we are told to exercise to “burn off the fat.” Although fat is a complicated mixture, it has approximately the formula C56H108O6. Calculate the volume of oxygen that must be consumed at 22 °C and 1.00 atm of pressure to “burn off ” 5.0 pounds of fat.
Calculate the mass of water produced in the reaction of 4.33 L oxygen and 6.77 L hydrogen gas. Both gases are at a pressure of 1.22 atm and a temperature of 27 °C.
Calculate(a) The rms speed (in m/s) of samples of hydrogen and nitrogen at STP; and(b) The average kinetic energies per molecule (in kg m2/s2) of the two gases under these conditions.
Lithium hydroxide is used to remove the CO2 produced by the respiration of astronauts. An astronaut produces about 400 L CO2 at 24 °C and 1.00 atm of pressure every 24 hours. What mass of lithium hydroxide, in grams, is needed to remove the CO2 produced by the astronaut in 24 hours? Th e equation
(a) Use the van der Waals equation to calculate the pressure, in atm, of 30.33 mol hydrogen at 240 °C in a 2.44-L container.(b) Do the same calculation for methane under the same conditions.(c) What difference between the two gases causes the pressure in the containers to be different?
The graphs below represent two plots of average speed of a gas versus the number of particles with that speed.(a) If one plot is for argon and the other neon, which plot would be for neon?(b) If both gases are the same, which plot represents the gas at a greater temperature? Speed Number of
Draw a plot similar to that shown above for the following:(a) Ar at 0 °C(b) Ar at 100 °C
For each of the following pairs of gases at the given conditions, predict which one would more closely follow the ideal gas law. Explain your choice.(a) Oxygen (boiling point = -183 °C) or sulfur dioxide (boiling point = -10 °C), both measured at 25 °C and 1 atm(b) Nitrogen (boiling point =
An effusion container is filled with 50 mL of an unknown gas, and it takes 163 seconds for the gas to effuse into a vacuum. From the same container, under the same conditions of constant pressure and temperature, it takes 103 seconds for 50 mL N2 gas to effuse. Calculate the molar mass of the
For the following pairs of gases at the given conditions, predict which one would more closely follow the ideal gas law. Explain your choice.(a) nitrogen (boiling point = -196 °C) or butane (boiling point = -1 °C), both measured at 25 °C and 1 atm(b) Oxygen gas at 0.50 atm or at 150 atm, both
Calculate the pressure, in atm, of 10.2 mol argon at 530 °C in a 3.23-L container, using both the ideal gas law and the van der Waals equation.
Calculate the pressure, in atm, of 1.55 mol nitrogen at 530 °C in a 3.23-L container, using both the ideal gas law and the van der Waals equation.
A 1.26-g sample of a gas occupies a volume of 544 mL at 27 °C and 744 torr? What is the molecular formula and name of the gas if its empirical formula is C2H5.
A 2.8-L tank is filled with 0.24 kg oxygen. What is the pressure in the tank at 20 °C? Assume ideal behavior.
For the following pairs of gases at the given conditions, predict which one would more closely follow the ideal gas law. Explain your choice.(a) CO2 gas at 0.05 atm or at 10 atm of pressure(b) Propane (boiling point = -45 °C) or neon (boiling point = -246 °C) gas at -20 °C and 1 atm(c) Sulfur
Calculate the pressure, in atm, of 5.75 mol methane (CH4) at 440 °C in a 4.93-L container, using both the ideal gas law and the van der Waals equation.
It is important to check the pressure in car tires at the start of the winter, because the large temperature change will cause the pressure to drop. Calculate the pressure change in a tire inflated to 32 pounds per square inch (psi) at 90 °F if the temperature declines to 32 °F. Assume that
Calculate the pressure, in atm, of 13.9 mol neon at 420 °C in a 4.73-L container, using both the ideal gas law and the van der Waals equation.
Workers at a research station in the Antarctic collected a sample of air to test for airborne pollutants. They collected the sample in a 1.00-L container at 764 torr and -20 °C. Calculate the pressure in the container when it was opened for analysis in a particulate-free clean room in a laboratory
Three bulbs are connected by tubing, and the tubing is evacuated. The volume of the tubing is 22.0 mL. The first bulb has a volume of 50.0 mL and contains 2.00 atm argon, the second bulb has a volume of 250 mL and contains 1.00 atm neon, and the third bulb has a volume of 25.0 mL and contains 5.00
An enzyme in yeast can convert pyruvic acid, C3H4O3, to CO2 and C2H4O. What volume of CO2 gas is produced from 0.113 g pyruvic acid if the gas is collected at 755 torr and 25 °C?
Diborane, B2H6, is a gas at 744.0 torr and 120.0 °C. It reacts violently with O2(g), yielding B2O3(s) and water vapor. The reaction is so energetic that it once was considered as a possible rocket fuel. What is ΔH for the reaction of 1 mol B2H6 if the reaction of 2.329 L of B2H6 under the above
A 10.0-L container is filled with 2.66 g H2 and 4.88 g Cl2, and heated to 111 °C. After a few days, the H2(g) and Cl2 (g) had reacted to form HCl (g), but some of one of the reactant gases remains because it is present in excess. What is the pressure in the container?
What is the abbreviated electron configuration for antimony, an element found in bullets, whose atomic number is 51?StrategyUse the periodic table to find the next lower noble gas and build on its electron configuration.
What is the abbreviated electron configuration of barium?
A compound that contains only hydrogen and carbon is burned in oxygen gas at 180 °C and 755 torr of pressure to produce 1.23 L H2O (g) and 0.984 L CO2(g). What is the empirical formula of the compound?
Combustion of a 4.33-g sample of a compound yielded 2.20 L CO2 gas at a temperature of 27 °C and a pressure of 0.99 atm. What is the percentage of carbon in the sample?
If a 100.0-mL sample of 0.88 M H2O2 (hydrogen peroxide) solution decomposes into oxygen gas and water, what volume of oxygen is produced at a temperature of 22 °C and a pressure of 0.971 atm?
What is the frequency (in s-1) of radiation that has a wavelength of 3.00 m? (This is in the range used for commercial FM radio transmission.)
The table in the introduction to this chapter shows that copper is a common component of bullets. A characteristic light emission of excited copper atoms occurs at 324.7 nm. What is the frequency of this light?StrategyBecause wavelength × frequency is equal to the speed of light, we can rearrange
Light with a wavelength of 450.0 nm strikes metallic cesium and ejects electrons with a kinetic energy of 1.22 × 10-19 J. What is the photoelectric threshold frequency (in s-1) for cesium?
The threshold frequency (ν0) that can dislodge an electron from metallic sodium is 5.51 × 1014 s-1.(a) What is the energy, in joules, of a photon with frequency of ν0?(b) What is the energy, in joules, of a photon with a wavelength of 430.0 nm ?(c) What is the kinetic energy, in joules, of an
Find the wavelength (in nm) of the next line in the Balmer series, with n1 = 2 and n2 = 5.
Calculate the wavelength (in nm) of the line in the hydrogen spectrum for n1 = 2 and n2 = 4 (the second line of the Balmer series).StrategyThe Rydberg equation is used to relate the wavelength of light to n1 and n2.
What is the velocity (in m/s) of neutrons that have a wavelength of 0.200 nm? The mass of a neutron is 1.67 × 10-27 kg.
Find the wavelength of electrons that have a velocity of 3.00 × 106 m/s .StrategyThe relationship between the wavelength of electrons and their velocity is given in the de Broglie equation.
What is the notation for the subshell with n = 3 and ℓ = 1?
Give the notation for each of the following orbitals that is an allowed combination. If it is not an allowed combination, explain why. (a) n = 2, l = 1, me = 0 (b) n = 5, l = 3, me = -3
Give the notation for each of the following orbitals that is an allowed combination of quantum numbers. If it is not an allowed combination, explain why.StrategyRemember that ℓ goes from 0 to (n - 1) and mℓ ranges from -ℓ to ℓ. (a) n = 3, l = 0, me = 0 (c) n = 2, l = 2, me = +1 (e) n = 3,
Find the wavelength of the light, in nanometers, emitted by an electron during a transition from the n = 3 to the n = 1 level in the C5+ ion.
What is the wavelength of light, in nanometers, required to raise an electron in the O7+ ion from the n = 1 shell to the n = 2 shell?StrategyUse Equation 7.8 and the knowledge that a photon must have the same energy as the difference in energies of two quantized energy levels. Note that for an
Bromine atoms have 35 electrons around the nucleus. What is the electron configuration of a bromine atom?StrategyUse Figure 7.21 to determine the order of filling of subshells beyond the 3p subshell. Fill subshells until the total number of electrons is 35.Figure 7.21 1s Is' 2s 3s 4s к 5s 75 3p
What is the electron configuration of Zr, whose atomic number is 40?
Give the notation for each of the following subshells that is an allowed combination of quantum numbers. If it is not an allowed combination, explain why.StrategyApply the rules for the possible values of n and ℓ. (a) n = 2, l = 0 (b) n = 1, l = 1 (c) n = 4, l = 2
In Example 3.15, the empirical formula of a compound extracted from tobacco was calculated to be C5H7N. In a separate experiment, the molar mass of this compound is found to be 162 g/mol. Calculate the molecular formula.StrategyThe molecular formula is determined from the empirical formula by
Use Equation 5.3 to determine the enthalpy change when 6.00 mol C2H6 burns in excess oxygen.Equation 5.3 2C₂H6(g) + 702(g) → 4CO₂(g) + 6H₂O(l) AH-3120 kJ
Calculate the enthalpy change if 5.00 mol N2 (g) reacts with O2 (g) to make NO, a toxic air pollutant and important industrial compound, using the following thermochemical equation:StrategyWe will use the same approach as used in previous stoichiometry problems, except that this time a
A reaction is conducted with 20.0 g H2 and 99.8 g O2.(a) State the limiting reactant.(b) Calculate the mass, in grams, of H2O that can be produced from this reaction.StrategyWe use the same four-step procedure outlined in Section 3.4, but we must calculate the quantities of product that could
The chapter introduction introduced the following reaction as one chemical reaction used to launch the space shuttle. Calculate the mass of aluminum required to generate 60,500 kJ energy (enough to launch 1 kg of matter into space). The thermochemical equation isStrategyThe approach is the reverse
Use Equation 5.2 to calculate the enthalpy change when 5.00 g O2 is consumed by reaction with N2, forming NO.Equation 5.2 N₂(g) + O₂(g) - → 2NO(g) ΔΗ = +181.8 kJ
Calculate the enthalpy change observed in the combustion reaction of 1.00 g ethane, using the thermochemical equation.Thermochemical EquationStrategyWe will use the same approach as in previous stoichiometry calculations. Convert the mass of ethane to moles; then use stoichiometric relations in the
Why must the physical states of all reactants and products be specified in a thermochemical equation?
This chapter’s introduction mentioned the following reaction as one chemical reaction used to power the lunar module in space. Calculate the mass of dinitrogen tetroxide, N2O4, required to generate 7632 J of energy (the approximate kinetic energy of the lunar module moving at a velocity of 1
Why is chemical energy classified as a form of potential energy?
What quantity of heat must be added to a 120-g sample of aluminum to change its temperature from 23.0 °C to 34.0 °C ?Strategy Use Equation 5.4 and the value of the specific heat of aluminum from Table 5.1 to determine the heat.Equation 5.4Table 5.1 g=mC AT mC.AT
What is the difference between the enthalpy of reaction and the enthalpy of formation? For what chemical reaction(s) are the two quantities the same?
Aluminum oxide is one material used to construct the nozzles in the engines of the space shuttle (see this chapter’s introduction). What quantity of heat is needed to increase the temperature of 1.20 × 102 g Al2O3 (Cs = 0.773 J/g · °C) by 11.0 °C?
Classify each process as exothermic or endothermic.(a) Ice melts(b) Gasoline burns(c) Steam condenses(d) Reactants → products, ΔH = -50 kJ
Explain why the specific heat of the contents of the calorimeter must be known in a calorimetry experiment.
When a 43.0-g sample of metal at 100.0 °C is added to 38.0 g water at 23.72 °C, the final temperature of both the metal and the water is 29.33 °C. The specific heat of water is 4.184 J/g · °C. What is the specific heat of the metal?
When a 60.0-g sample of metal at 100.0 °C is added to 45.0 g water at 22.60 °C , the final temperature of both the metal and the water is 32.81 °C . The specific heat of water is 4.184 J/g · °C . Calculate the specific heat of the metal.StrategyBecause of the law of conservation of energy, the
Define energy. What are its units?
A 50.0-g sample of a dilute acid solution is added to 50.0 g of a base solution in a coffee-cup calorimeter. The temperature of the liquid increases from 18.20 °C to 21.30 °C . Calculate q for the neutralization reaction, assuming that the specific heat of the solution is the same as that of
A chemical reaction releases enough heat to increase the temperature of 49.9 g water from 17.82 °C to 19.72 °C. Calculate q for the reaction.
The reaction of 0.440 g magnesium with 400 g (excess) hydrochloric acid solution causes the temperature of the solution to increase by 5.04 °C. Assume that the specific heat of the solution is the same as that of water, and Mg is the limiting reactant. Calculate the ΔH for the reaction as
Define heat. What are its units? How does it differ from energy?
A 50.0 g-sample of acid takes 46.4 mL of 0.500 M NaOH solution to neutralize it. Assume the same amount of heat is given off as in Example 5.6.(a) Calculate the enthalpy change for the neutralization per mole of hydrogen ions, described by the equation(b) Is the neutralization reaction an
Calculate the enthalpy change forusing the thermochemical equations C2H,(g) + HO(0) → CHOH(0) ΔΗ = ?
Hydrogenation of hydrocarbons is an important reaction in the chemical industry. A simple example is the hydrogenation of ethylene to form ethane. Calculate the enthalpy change for Use the following thermochemical equations to determine the overall enthalpy change.StrategyIdentify the position of
Differentiate between kinetic energy and potential energy.
Th e chemical industry converts hydrocarbons of low molecular mass to larger and more useful compounds. Calculate the change in enthalpy for the synthesis of cyclohexane (C6H12), a compound used in the production of nylon, from ethylene.Use the information in Example 5.8 and the thermochemical
Given the thermochemical equations Sn(s) + Cl₂(g) → SnCl₂(s) SnCl,(s) + Cl,(g) → SnCl(0) determine AH for 2SnCl₂(s)→ Sn(s) + SnC14(0) AH = -325 kJ ΔΗ = − 186 kJ - AH = ?
Describe the difference between the system and the surroundings.
What characteristic does every exothermic reaction have?
Which of the following reactions are formation reactions? (a) H₂(g) + O(g) → H₂O(g) (b) Fe(s) + N₂(g) + 302(g) → Fe(NO3)2(s) 3. (c)NH₂(g) →N₂(g) + H₂(g) 2 2
Which of the following reactions are formation reactions?StrategyLook for reactions that have all elements in their standard states as reactants and one mole of a compound as a product. (a) 2H₂(g) + O₂(g) → 2H₂O(1) (b) Fe₂O3(s) + 3SO3(g) → Fe₂(SO4)3(s) (c) N₂(g) + H₂(g) →
One step in the production of nitric acid, a powerful acid used in the production of fertilizers and explosives, is the combustion of ammonia.Use Equation 5.10, with the enthalpies of formation of these substances in Table 5.2, to find of this reaction.Equation 5.10Table 5.2StrategyLook up the
Write the correct formation reactions for the following substances. Consult a periodic table for the proper phases of the elements involved. (a) C6H6(l) (b) C6H12O6(s) (c) BaCO3(s)
What characteristic does every endothermic reaction have?
Write the correct formation reactions for the following substances. Consult a periodic table for the proper phases of the elements involved.StrategyWrite chemical reactions for the formation of one mole of the given substance, with the reactants being the constituent elements of the substance in
Another step in the production of nitric acid is the conversion of nitrogen monoxide to nitrogen dioxide. Using enthalpies of formation from Appendix G, calculate the enthalpy change that accompanies the reaction O₂(g) →→→ 2NO2(g) 2NO(g) + O₂(g).
Is the Sun exothermic or endothermic? Is it any less exothermic or endothermic in the winter, as opposed to the summer?
Calculate the standard enthalpy of formation for glucose, C6H12O6(s), from the following information. A calorimetry experiment shows that the enthalpy of combustion of 1 mol glucose to form carbon dioxide and water at 298.15 K is -2807.8 kJ. Use the data in Table 5.2 for the standard enthalpies of
Th e standard enthalpy change when 1 mol rubbing alcohol, isopropanol, , burns to form carbon dioxide and liquid water at 298.15 K is -2005.8 kJ. Calculate the standard enthalpy of formation of rubbing alcohol. C3H₂OH(l),
Under what circumstances is the heat of a process equal to the enthalpy change for the process?
Cheryl walks upstairs from the lobby of her residence hall to the roof, where she studies chemistry in the open air. She is joined by Carol, who rode the elevator from the lobby. Consider the two students’ journeys, and identify which of the following are state functions and which are path
State in words the meaning of the following thermochemical equation: C₂H4(g) + 30₂(g) →2CO₂(g) + 2H₂O(1) AH = -1411 kJ
State the first law of thermodynamics.
Draw an enthalpy diagram for reactants → products that illustrates the use of enthalpies of formation in the calculation of the enthalpy change for the reaction. The diagram should have three levels—one for reactants, one for products, and one for the free elements. Draw arrows between the
Draw an energy-level diagram for an exothermic reaction of the following type:reactants → products
Draw an energy-level diagram for an endothermic reaction of the following type:reactants → products
Th e formation of hydrogen chloride is exothermic:What are the values of for H₂(g) + Ch₂(g) - Cl₂(g) → HCl(g) ΔΗ = −92.3 kJ
Methane, CH4(g), and octane, , are important components of the widely used fossil fuels. Th e enthalpy change for combustion of 1 mol methane is -890 kJ, and that for 1 mol octane is -5466 kJ. Which of these fuels produces more energy per gram of compound burned? What is the difference in energy
Explain why absolute enthalpies cannot be measured and only changes can be determined.
Addition of solid ammonium nitrate to water in a coffee cup calorimeter results in a solution with a temperature lower than the original temperature of the water. The NH4NO3(s) absorbs heat in the process of dissolving,If the calorimeter is perfectly insulating (no heat can enter or leave), what
Describe how Hess’s law leads to Equation 5.10. Use the reactionto justify your description.Equation 5.10 2NaHCO3(s) → Na₂CO3(s) + H₂O() + CO₂(g)
Explain why the calorimeter and its contents are the only part of the surroundings that are used to calculate the ΔH of reaction.
Under what conditions can the value of ΔH for a reaction be denoted by the symbol ΔH°?
Why is it unnecessary to include the enthalpies of formation of elements, such as P4(s), H2(g), or C(graphite), in a table of standard enthalpies of formation?
A toaster toasts some bread at high temperature, then cools. After it has cooled down, the kitchen is found to have warmed up by 0.024 °C. Identify the system, the surroundings, and indicate whether the process that has occurred was exothermic or endothermic.

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