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chemistry
physical chemistry

General Chemistry 9th edition Darrell Ebbing, Steven D. Gammon - Solutions

If it takes 10.6 hours for 1.00 L of nitrogen, N2, to effuse through the pores in a balloon, how long would it take for 1.00 L of helium, He, to effuse under the same conditions?
If 4.83 mL of an unknown gas effuses through a hole in a plate in the same time it takes 9.23 mL of argon, Ar, to effuse through the same hole under the same conditions, what is the molecular mass of the unknown gas?
An electron, whose mass is 9.11 × 10–31 kg, is accelerated by a positive charge to a speed of 5.0 × 106 m/s. What is the kinetic energy of the electron in joules? in calories?
Calculate the enthalpy change for the following reaction:3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) Use standard enthalpies of formation.
Calculate the standard enthalpy change for the reaction of an aqueous solution of barium hydroxide, Ba(OH)2, with an aqueous solution of ammonium nitrate, NH4NO3, at 25oC. (Figure 6.1 illustrated this reaction using solids instead of solutions.) The complete ionic equation isBa2+(aq) + 2OH(aq) +
A propellant for rockets is obtained by mixing the liquids hydrazine, N2H4, and dinitrogen tetroxide, N2O4. These compounds react to give gaseous nitrogen, N2, and water vapor, evolving 1049 kJ of heat at constant pressure when 1 mol N2O4 reacts. Write the thermochemical equation for this reaction.
a. Write the thermochemical equation for the reaction described in Exercise 6.3 for the case involving 1 mol N2H4. b. Write the thermochemical equation for the reverse of the reaction described in Exercise 6.3.
How much heat evolves when 10.0 g of hydrazine reacts according to the reaction described in Exercise 6.3?
Iron metal has a specific heat of 0.449 J/(g•oC). How much heat is transferred to a 5.00-g piece of iron, initially at 20.0oC, when it is placed in a pot of boiling water? Assume that the temperature of the water is 100.0oC and that the water remains at this temperature, which is the final
Suppose 33 mL of 1.20 M HCl is added to 42 mL of a solution containing excess sodium hydroxide, NaOH, in a coffee-cup calorimeter. The solution temperature, originally 25.0oC, rises to 31.8oC. Give the enthalpy change, ∆H, for the reaction HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) Express the
Manganese metal can be obtained by reaction of manganese dioxide with aluminum.4Al(s) + 3MnO2(s) †’ 2Al2O3(s) + 3Mn(s)What is ˆ†H for this reaction? Use the following data:
Calculate the heat of vaporization, ˆ†Hovap, of water, using standard enthalpies of formation (Table 6.2).
A solar-powered water pump has photovoltaic cells that protrude from top panels. These cells collect energy from sunlight, storing it momentarily in a battery, which later runs an electric motor that pumps water up to a storage tank on a hill. What energy conversions are involved in using sunlight
Natural gas consists primarily of methane, CH4. It is used in a process called steam reforming to prepare a gaseous mixture of carbon monoxide and hydrogen for industrial use. CH4(g) + H2O(g) → CO(g) + 3H2(g); H × 206 kJ The reverse reaction, the reaction of carbon monoxide and hydrogen, has
The heat of fusion (also called heat of melting), ∆Hfus, of ice is the enthalpy change for H2O(s) → H2O(l); ∆Hfus Similarly, the heat of vaporization, ∆Hvap, of liquid water is the enthalpy change for H2O(l) → H2O(g); ∆Hvap How is the heat of sublimation, ∆Hsub, the enthalpy change
Define energy, kinetic energy, potential energy, and internal energy.
The specific heat of copper metal was determined by putting a piece of the metal weighing 35.4 g in hot water. The quantity of heat absorbed by the metal was calculated to be 47.0 J from the temperature drop of the water. What was the specific heat of the metal if the temperature of the metal rose
A 50.0-g sample of water at 100.00oC was placed in an insulated cup. Then 25.3 g of zinc metal at 25.00oC was added to the water. The temperature of the water dropped to 96.68C. What is the specific heat of zinc?
A 19.6-g sample of a metal was heated to 61.67oC. When the metal was placed into 26.7 g of water in a calorimeter, the temperature of the water increased from 25.00oC to 30.00oC. What is the specific heat of the metal?
A 14.1-mL sample of 0.996 M NaOH is mixed with 32.3 mL of 0.905 MHCl in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole number coefficients, is 55.8 kJ. Both solutions are at 21.6oC
A 29.1-mL sample of 1.05 M KOH is mixed with 20.9 mL of 1.07 M HBr in a coffee-cup calorimeter. The enthalpy of the reaction, written with the lowest whole number coefficients, is 55.8 kJ. Both solutions are at 21.8oC prior to mixing and reacting. What is the final temperature of the reaction
In a calorimetric experiment, 6.48 g of lithium hydroxide, LiOH, was dissolved in water. The temperature of the calorimeter rose from 25.00oC to 36.66oC. What is H for the solution process? LiOH(s) → Li+(aq) + OH(aq) The heat capacity of the calorimeter and its contents is 547 J/oC.
When 21.45 g of potassium nitrate, KNO3, was dissolved in water in a calorimeter, the temperature fell from 25.00oC to 14.14oC. What is the H for the solution process? KNO3(s) → K+(aq) + NO3(aq) The heat capacity of the calorimeter and its contents is 682 J/oC.
A 10.00-g sample of acetic acid, HC2H3O2, was burned in a bomb calorimeter in an excess of oxygen. HC2H3O2(l) + 2O2(g) → 2CO2(g) + 2H2O(l) The temperature of the calorimeter rose from 25.00oC to 35.84oC. If the heat capacity of the calorimeter and its contents is 13.43 kJ/oC, what is the enthalpy
The sugar arabinose, C5H10O5, is burned completely in oxygen in a calorimeter. C5H10O5(s) + 5O2(g) → 5CO2(g) + 5H2O(l) Burning a 0.548-g sample caused the temperature to rise from 20.00oC to 20.54oC. The heat capacity of the calorimeter and its contents is 15.8 kJ/oC. Calculate ∆H for the
Hydrogen sulfide, H2S, is a poisonous gas with the odor of rotten eggs. The reaction for the formation of H2S from the elements isUse Hess€™s law to obtain the enthalpy change for this reaction from the following enthalpy changes:
Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2H4O, by the reactionC2H4O(g) + H2O(l) †’ HOCH2CH2OH(l)Use Hess€™s law to obtain the enthalpy change for this reaction from the following enthalpy changes:
Hydrogen, H2, is prepared by steam reforming, in which hydrocarbons are reacted with steam. For CH4, CH4(g) + H2O(g) → CO(g) + 3H2(g) Calculate the enthalpy change ∆Ho for this reaction, using standard enthalpies of formation.
Hydrogen is prepared from natural gas (mainly methane, CH4) by partial oxidation. 2CH4(g) + O2(g) → 2CO(g) + 4H2(g) Calculate the enthalpy change ∆Ho for this reaction, using standard enthalpies of formation.
Calcium oxide, CaO, is prepared by heating calcium carbonate (from limestone and seashells). CaCO3(s) → CaO(s) + CO2(g) Calculate the standard enthalpy of reaction, using enthalpies of formation. The ∆Hof of CaO(s) is 635 kJ/mol. Other values are given in Table 6.2.
Sodium carbonate, NA2CO3, is used to manufacture glass. It is obtained from sodium hydrogen carbonate, NaHCO3, by heating.2NaHCO3(s) †’ NA2CO3(s) + H2O(g) + CO2(g)Calculate the standard enthalpy of reaction, using enthalpies of formation (Table 6.2).
Calculate the heat released when 2.000 L O2 with a density of 1.11 g/L at 25oC reacts with an excess of hydrogen to form liquid water at 25oC.
Calculate the heat released when 4.000 L Cl2 with a density of 2.46 g/L at 25oC reacts with an excess of sodium metal to form solid sodium chloride at 25oC.
Sucrose, C12H22O11, is common table sugar. The enthalpy change at 25oC and 1 atm for the complete burning of 1 mol of sucrose in oxygen to give CO2(g) and H2O(l) is –5641 kJ. From this and from data given in Table 6.2, calculate the standard enthalpy of formation of sucrose.
Acetone, CH3COCH3, is a liquid solvent. The enthalpy change at 25oC and 1 atm for the complete burning of 1 mol of acetone in oxygen to give CO2(g) and H2O(l) is €“1791 kJ. From this and from data given in Table 6.2, calculate the standard enthalpy of formation of acetone.
Ammonium nitrate is an oxidizing agent and can give rise to explosive mixtures. A mixture of 2.00 mol of powdered aluminum and 3.00 mol of ammonium nitrate crystals reacts exothermically, yielding nitrogen gas, water vapor, and aluminum oxide. How many grams of the mixture are required to provide
Consider the reaction of methane, CH4, with oxygen, O2, discussed in Section 6.5. How would you set up the calculation if the problem had been to compute the heat if 10.0 g H2O were produced (instead of 10.0 g CH4 reacted)?
The thermite reaction is a very exothermic reaction; it has been used to produce liquid iron for welding. A mixture of 2 mol of powdered aluminum metal and 1 mol of iron(III) oxide yields liquid iron and solid aluminum oxide. How many grams of the mixture are needed to produce 348 kJ of heat? See
Describe the physical characteristics of white phosphorus. Is it found in any modern matches? Why or why not?
What is the phosphorus compound used in “strike anywhere” matches. What is the chemical equation for the burning of this compound in air?
How fast (in meters per second) must an iron ball with a mass of 56.6 g be traveling in order to have a kinetic energy of 15.75 J? The density of iron is 7.87 g/cm3.
Sulfur dioxide gas reacts with oxygen, O2(g), to produce SO3(g). This reaction releases 99.0 kJ of heat (at constant pressure) for each mole of sulfur dioxide that reacts. Write the thermochemical equation for the reaction of 2 mol of sulfur dioxide, and then also for the decomposition of 3 mol of
When solid iron burns in oxygen gas (at constant pressure) to produce Fe2O3(s), 1651 kJ of heat is released for every 4 mol of iron burned. How much heat is released when 10.3 g Fe2O3(s) is produced (at constant pressure)? What additional information would you need to calculate the heat released to
How many grams of oxygen gas are required to produce 7.60 kJ of heat when hydrogen gas burns at constant pressure to produce gaseous water? 2H2(g) + O2(g) → 2H2O(g); ∆H = –484 kJ Liquid water has a heat of vaporization of 44.0 kJ per mole at 25C.
A piece of iron was heated to 95.4oC and dropped into a constant-pressure calorimeter containing 284 g of water at 32.2oC. The final temperature of the water and iron was 51.9oC. Assuming that the calorimeter itself absorbs a negligible amount of heat, what was the mass (in grams) of the piece of
The enthalpy of combustion, ∆H, for benzoic acid, C6H5COOH, is –3226 kJ/mol. When a sample of benzoic acid was burned in a calorimeter (at constant pressure), the temperature of the calorimeter and contents rose from 23.44oC to 27.65oC. The heat capacity of the calorimeter and contents was
Define the heat capacity of a substance. Define the specific heat of a substance.
Given the following (hypothetical) thermochemical equations: A + B → 2C; ∆H = –447 kJ A + 3D → 2E; ∆H = –484 kJ 2D + B → 2F; ∆H = –429 kJ Calculate ∆H, in kJ, for the equation 4E + 5B → 4C + 6F
The head of a “strike anywhere” match contains tetraphosphorus trisulfide, P4S3. In an experiment, a student burned this compound in an excess of oxygen and found that it evolved 3651 kJ of heat per mole of P4S3 at a constant pressure of 1 atm. She wrote the following thermochemical
Toluene, C6H5CH3, has an enthalpy of combustion of –3908 kJ/mol. Using data from Appendix C, calculate the enthalpy of formation of toluene.
What will be the final temperature of a mixture made from 25.0 g of water at 15.0oC, from 45.0 g of water at 50.0oC, and from 15.0 g of water at 37.0oC?
What will be the final temperature of a mixture made from equal masses of the following: water at 25.0oC, ethanol at 35.5oC, and iron at 95oC?
Graphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is 33% CO and 67% CO2 by mass, what is the heat from the combustion of 1.00 g of graphite?
A sample of natural gas is 80.0% CH4 and 20.0% C2H6 by mass. What is the heat from the combustion of 1.00 g of this mixture? Assume the products are CO2(g) and H2O(l).
A sample containing 2.00 mol of graphite reacts completely with a limited quantity of oxygen at 25oC and 1.0 atm pressure, producing 481 kJ of heat and a mixture of CO and CO2. Calculate the masses of CO and CO2 produced.
A 10.0-g sample of a mixture of CH4 and C2H4 reacts with oxygen at 25oC and 1 atm to produce CO2(g) and H2O(l). If the reaction produces 520 kJ of heat, what is the mass percentage of CH4 in the mixture?
How much heat is released when a mixture containing 10.0 g NH3 and 20.0 g O2 reacts by the following equation? 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g); ∆H° = –906 kJ
Describe a simple calorimeter. What measurements are needed to determine the heat of reaction?
How much heat is released when a mixture containing 10.0 g CS2 and 10.0 g Cl2 reacts by the following equation? CS2(g) + 3Cl2(g) → S2Cl2(g) + CCl4(g); ∆H° = –230 kJ
Consider the Haber process: N2(g) + 3H2(g) → 2NH3(g); ∆H° = –91.8 kJ The density of ammonia at 25oC and 1.00 atm is 0.696 g/L. The density of nitrogen, N2, is 1.145 g/L, and the molar heat capacity is 29.12 J/(mol•oC). (a) How much heat is evolved in the production of 1.00 L of ammonia at
An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g) + 3O2(g) → 2H2O(l ) + 2SO2(g); ∆H° = –1124 kJ The density
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide. 2LiOH(s) + CO2(g) → Li2CO3(s) + H2O(l ) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 × 103 kcal of
A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s) + 2H2O(l) → 4KOH(s) + 3O2(g) Estimate the grams of potassium superoxide required to supply a person’s oxygen needs for one hour. Assume a person requires 1.00 × 102 kcal
What property of enthalpy provides the basis of Hess’slaw? Explain.
You discover that you cannot carry out a particular reaction for which you would like the enthalpy change. Does this mean that you will be unable to obtain this enthalpy change? Explain.
What is meant by the reference form of an element? What is the standard enthalpy of formation of an element in its reference form?
What is meant by the standard enthalpy of formation of a substance?
Write the chemical equation for the formation reaction of H2S(g).
Is the following reaction the appropriate one to use in determining the enthalpy of formation of methane, CH4(g)? Why or why not? C(g) + 4H(g) → CH4(g)
What is a fuel? What are the fossil fuels?
Give chemical equations for the conversion of carbon in coal to methane, CH4.
List some rocket fuels and corresponding oxidizers. Give thermochemical equations for the exothermic reactions of these fuels with the oxidizers.
Part 1: In an insulated container, you mix 200. g of water at 80oC with 100. g of water at 20oC. After mixing, the temperature of the water is 60oC.a. How much did the temperature of the hot water change? How much did the temperature of the cold water change? Compare the magnitudes (positive
a. A 100.-g sample of water is placed in an insulated container and allowed to come to room temperature at 21oC. To heat the water sample to 41oC, how much heat must you add to it? b. Consider the hypothetical reaction,2X(aq) + Y(l) → X2Y(aq)
A small car is traveling at twice the speed of a larger car, which has twice the mass of the smaller car. Which car has the greater kinetic energy? (Or do they both have the same kinetic energy?)
The equation for the combustion of butane, C4H10, isWhich one of the following generates the least heat? Why? a. Burning one mole of butane b. Reacting one mole of oxygen with excess butane c. Producing one mole of carbon dioxide by burning butane d. Producing one mole of water by burning butane
A 250-g sample of water at 20.0oC is placed in a freezer that is held at a constant temperature of 20.0oC. Considering the water as the “system,” answer the following questions: a. What is the sign of qsys for the water after it is placed in the freezer? b. After a few hours, what will be the
A 20.0-g block of iron at 50.0oC and a 20.0 g block of aluminum at 45oC are placed in contact with each other. Assume that heat is only transferred between the two blocks.a. Draw an arrow indicating the heat flow between the blocks. b. What is the sign of qsys for the aluminum when the blocks first
What is the enthalpy change for the preparation of one mole of liquid water from the elements, given the following equations?
A block of aluminum and a block of iron, both having the same mass, are removed from a freezer and placed outside on a warm day. When the same quantity of heat has flowed into each block, which block will be warmer? Assume that neither block has yet reached the outside temperature.
You have two samples of different metals, metal A and metal B, each having the same mass. You heat both metals to 95oC and then place each one into separate beakers containing the same quantity of water at 25oC. a. You measure the temperatures of the water in the two beakers when each metal has
Consider the reactions of silver metal, Ag(s), with each of the halogens: fluorine, F2(g), chlorine, Cl2(g), and bromine, Br2(l). What chapter data could you use to decide which reaction is most exothermic? Which reaction is that?
Tetraphosphorus trisulfide, P4S3, burns in excess oxygen to give tetraphosphorus decoxide, P4O10, and sulfur dioxide, SO2. Suppose you have measured the enthalpy change for this reaction. How could you use it to obtain the enthalpy of formation of P4S3? What other data do you need?
Describe the interconversions of potential and kinetic energy in a moving pendulum. A moving pendulum eventually comes to rest. Has the energy been lost? If not, what has happened to it?
A soluble salt, MX2, is added to water in a beaker. The equation for the dissolving of the salt is: MX2(s) → M2+(aq) + 2X(aq); ∆H > 0
Methane, CH4, is a major component of marsh gas. When 0.5000 mol methane burns to produce carbon dioxide and liquid water, –445.1 kJ of heat is released. What is this heat in kilocalories?
Hydrogen sulfide, H2S, is produced during decomposition of organic matter. When 0.5500 mol H2S burns to produce SO2(g) and H2O(l), –309.1 kJ of heat is released. What is this heat in kilocalories?
A car whose mass is 4.85 Ã— 103 lb is traveling at a speed of 57 miles per hour. What is the kinetic energy of the car in joules? in calories? See Table 1.4 for conversion factors.
A bullet weighing 245 grains is moving at a speed of 2.52 × 103 ft/s. Calculate the kinetic energy of the bullet in joules and in calories. One grain equals 0.0648 g.
Chlorine dioxide, ClO2, is a reddish yellow gas used in bleaching paper pulp. The average speed of a ClO2 molecule at 25oC is 306 m/s. What is the kinetic energy (in joules) of a ClO2 molecule moving at this speed?
Nitrous oxide, N2O, has been used as a dental anesthetic. The average speed of an N2O molecule at 25oC is 379 m/s. Calculate the kinetic energy (in joules) of an N2O molecule traveling at this speed.
Nitric acid, a source of many nitrogen compounds, is produced from nitrogen dioxide. An old process for making nitrogen dioxide employed nitrogen and oxygen. N2(g) + 2O2(g) → 2NO2(g) The reaction absorbs 66.2 kJ of heat per 2 mol NO2 produced. Is the reaction endothermic or exothermic? What is
Hydrogen cyanide is used in the manufacture of clear plastics such as Lucite and Plexiglas. It is prepared from ammonia and natural gas (CH4). 2NH3(g) + 3O2(g) + 2CH4(g) → 2HCN(g) + 6H2O(g) The reaction evolves 939 kJ of heat per 2 mol HCN formed. Is the reaction endothermic or exothermic? What
When 1 mol of iron metal reacts with hydrochloric acid at constant temperature and pressure to produce hydrogen gas and aqueous iron(II) chloride, 89.1 kJ of heat evolves. Write a thermochemical equation for this reaction.
When 2 mol of potassium chlorate crystals decompose to potassium chloride crystals and oxygen gas at constant temperature and pressure, 78.0 kJ of heat is given off. Write a thermochemical equation for this reaction.
When white phosphorus burns in air, it produces phosphorus (V) oxide.P4(s) + 5O2(g) †’ P4O10(s); ˆ†H = €“3010 kJWhat is ˆ†H for the following equation?P4O10(s) †’ P4(s) + 5O2(g)
Carbon disulfide burns in air, producing carbon dioxide and sulfur dioxide.CS2(l) + 3O2(g) †’ CO2(g) + 2SO2(g); ˆ†H = €“1077 kJWhat is ˆ†H for the following equation?
Phosphoric acid, H3PO4, can be prepared by the reaction of phosphorus(V) oxide, P4O10, with water.What is ˆ†H for the reaction involving 1 mol of P4O10? P4O10(s) + 6H2O(l ) †’ 4H3PO4(aq)
With a platinum catalyst, ammonia will burn in oxygen to give nitric oxide, NO.4NH3(g) + 5O2(g) †’ 4NO(g) + 6H2O(g);ˆ†H = €“906 kJWhat is the enthalpy change for the following reaction?
Colorless nitric oxide, NO, combines with oxygen to form nitrogen dioxide, NO2, a brown gas. 2NO(g) + O2(g) → 2NO2(g); ∆H = –114 kJ What is the enthalpy change per gram of nitric oxide?

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