All Matches
Solution Library
Expert Answer
Textbooks
Search Textbook questions, tutors and Books
Oops, something went wrong!
Change your search query and then try again
Toggle navigation
FREE Trial
S
Books
FREE
Tutors
Study Help
Expert Questions
Accounting
General Management
Mathematics
Finance
Organizational Behaviour
Law
Physics
Operating System
Management Leadership
Sociology
Programming
Marketing
Database
Computer Network
Economics
Textbooks Solutions
Accounting
Managerial Accounting
Management Leadership
Cost Accounting
Statistics
Business Law
Corporate Finance
Finance
Economics
Auditing
Ask a Question
Search
Search
Sign In
Register
study help
chemistry
physical chemistry
Questions and Answers of
Physical Chemistry
Determine the oxidation numbers of all the elements in each of the following compounds. a. Hg2(BrO3)2 b. Cr2(SO4)3 c. CoSeO4 d. Pb(OH)2
In the following reactions, label the oxidizing agent and the reducing agent. a. P4(s) + 5O2(g) → P4O10(s) b. Co(s) + Cl2(g) → CoCl2(s)
In the following reactions, label the oxidizing agent and the reducing agent. a. ZnO(s) + C(s) → Zn(g) + CO(g) b. 8Fe(s) + S8(s) → 8FeS(s)
In the following reactions, label the oxidizing agent and the reducing agent. a. 2Al(s) + 3F2(g) → 2AlF3(s) b. Hg2+(aq) + NO2(aq) + H2O(l) → Hg(s) + 2H+(aq) + NO3(aq)
In the following reactions, label the oxidizing agent and the reducing agent. a. Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) b. PbS(s) + 4H2O2(aq) → PbSO4(s) + 4H2O(l)
Balance the following oxidation–reduction reactions by the half-reaction method.a. CuCl2(aq) + Al(s) → AlCl3(aq) + Cu(s)b. Cr3+(aq) + Zn(s) → Cr(s) + Zn2+(aq)
Balance the following oxidation–reduction reactions by the half-reaction method. a. FeI3(aq) + Mg(s) → Fe(s) + MgI2(aq) b. H2(g) + Ag+(aq) → Ag(s) + H+(aq)
A sample of 0.0512 mol of iron(III) chloride, FeCl3, was dissolved in water to give 25.0 mL of solution. What is the molarity of the solution?
A 50.0-mL volume of AgNO3 solution contains 0.0285 mol AgNO3 (silver nitrate). What is the molarity of the solution?
An aqueous solution is made from 0.798 g of potassium permanganate, KMnO4. If the volume of solution is 50.0 mL, what is the molarity of KMnO4 in the solution?
What are the major types of chemical reactions? Give a brief description and an example of each.
A sample of oxalic acid, H2C2O4, weighing 1.192 g is placed in a 100.0-mL volumetric flask, which is then filled to the mark with water. What is the molarity of the solution?
Heme, obtained from red blood cells, binds oxygen, O2. How many moles of heme are there in 150 mL of 0.0019 Mheme solution?
Insulin is a hormone that controls the use of glucose in the body. How many moles of insulin are required to make up 28 mL of 0.0048 M insulin solution?
How many grams of sodium dichromate, Na2Cr2O7, should be added to a 100.0-mL volumetric flask to prepare 0.025 M Na2Cr2O7 when the flask is filled to the mark with water?
Describe how you would prepare 2.50 × 102 mL of 0.20 M Na2SO4. What mass (in grams) of sodium sulfate, Na2SO4, is needed?
You wish to prepare 0.12 M HNO3 from a stock solution of nitric acid that is 15.8 M. How many milliliters of the stock solution do you require to make up 1.00 L of 0.12 M HNO3?
Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.
A chemist wants to prepare 0.50 M HCl. Commercial hydrochloric acid is 12.4 M. How many milliliters of the commercial acid does the chemist require to make up 1.50 L of the dilute acid?
A 3.50 g sample of KCl is dissolved in 10.0 mL of water. The resulting solution is then added to 60.0 mL of a 0.500 M CaCl2(aq) solution. Assuming that the volumes are additive, calculate the
Calculate the concentrations of each ion present in a solution that results from mixing 50.0 mL of a 0.20 M NaClO3(aq) solution with 25.0 mL of a 0.20 M Na2SO4(aq). Assume that the volumes are
A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ion as barium sulfate, BaSO4. How many grams of barium ion are in a 458-mg
A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to precipitate all of the iodide ion as silver iodide, AgI. If 1.545 g of the soluble iodide gave 2.185 g
Copper has compounds with copper(I) ion or copper(II) ion. A compound of copper and chlorine was treated with a solution of silver nitrate, AgNO3, to convert the chloride ion in the compound to a
Gold has compounds containing gold(I) ion or gold(III) ion. A compound of gold and chlorine was treated with a solution of silver nitrate, AgNO3, to convert the chloride ion in the compound to a
A compound of iron and chlorine is soluble in water. An excess of silver nitrate was added to precipitate the chloride ion as silver chloride. If a 134.8-mg sample of the compound gave 304.8 mg AgCl,
A 1.345-g sample of a compound of barium and oxygen was dissolved in hydrochloric acid to give a solution of barium ion, which was then precipitated with an excess of potassium chromate to give 2.012
What volume of 0.250 M HNO3 (nitric acid) reacts with 44.8 mL of 0.150 M Na2CO3 (sodium carbonate) in the following reaction? 2HNO3(aq) + Na2CO3(aq) → 2NaNO3(aq) + H2O(l ) + CO2(g)
Give an example of a neutralization reaction. Label the acid, base, and salt.
A flask contains 49.8 mL of 0.150 M Ca(OH)2 (calcium hydroxide). How many milliliters of 0.350 M Na2CO3 (sodium carbonate) are required to react completely with the calcium hydroxide in the following
How many milliliters of 0.150 M H2SO4 (sulfuric acid) are required to react with 8.20 g of sodium hydrogen carbonate, NaHCO3, according to the following equation? H2SO4(aq) + 2NaHCO3(aq) →
How many milliliters of 0.250 M KMnO4 are needed to react with 3.36 g of iron(II) sulfate, FeSO4? The reaction is as follows: 10FeSO4(aq) + 2KMnO4(aq) + 8H2SO4(aq) → 5Fe2(SO4)3(aq) + 2MnSO4(aq) +
A solution of hydrogen peroxide, H2O2, is titrated with a solution of potassium permanganate, KMnO4. The reaction is 5H2O2(aq) + 2KMnO4(aq) + 3H2SO4(aq) → 5O2(g) + 2MnSO4(aq) + K2SO4(aq) + 8H2O(l
A 3.33-g sample of iron ore is transformed to a solution of iron(II) sulfate, FeSO4, and this solution is titrated with 0.150 M K2Cr2O7 (potassium dichromate). If it requires 43.7 mL of potassium
Magnesium metal reacts with hydrobromic acid to produce hydrogen gas and a solution of magnesium bromide. Write the molecular equation for this reaction. Then write the corresponding net ionic
Aluminum metal reacts with perchloric acid to produce hydrogen gas and a solution of aluminum perchlorate. Write the molecular equation for this reaction. Then write the corresponding net ionic
Nickel(II) sulfate solution reacts with lithium hydroxide solution to produce a precipitate of nickel(II) hydroxide and a solution of lithium sulfate. Write the molecular equation for this reaction.
Potassium sulfate solution reacts with barium bromide solution to produce a precipitate of barium sulfate and a solution of potassium bromide. Write the molecular equation for this reaction. Then
Decide whether a reaction occurs for each of the following. If it does not, write NR after the arrow. If it does, write the balanced molecular equation; then write the net ionic equation. a. LiOH +
A gas in a container had a measured pressure of 57 kPa. Calculate the pressure in units of atm and mmHg.
A 10.0-L flask contains 1.031 g O2 and 0.572 g CO2 at 18oC. What are the partial pressures of oxygen and carbon dioxide? What is the total pressure? What is the mole fraction of oxygen in the mixture?
Oxygen can be prepared by heating potassium chlorate, KClO3, with manganese dioxide as a catalyst. The reaction isHow many moles of O2 would be obtained from 1.300 g KClO3? If this amount of O2 were
What is the rms speed (in m/s) of a carbon tetrachloride molecule at 22oC?
At what temperature do hydrogen molecules, H2, have the same rms speed as nitrogen molecules, N2, at 455oC? At what temperature do hydrogen molecules have the same average kinetic energy?
If it takes 3.52 s for 10.0 mL of helium to effuse through a hole in a container at a particular temperature and pressure, how long would it take for 10.0 mL of oxygen, O2, to effuse from the same
If it takes 4.67 times as long for a particular gas to effuse as it takes hydrogen under the same conditions, what is the molecular mass of the gas? (The rate of effusion is inversely proportional to
Use the van der Waals equation to calculate the pressure of 1.000 mol ethane, C2H6, that has a volume of 22.41 L at 0.0oC. Compare the result with the value predicted by the ideal gas law.
A volume of carbon dioxide gas, CO2, equal to 20.0 L was collected at 23oC and 1.00 atm pressure. What would be the volume of carbon dioxide collected at 23oC and 0.830 atm?
If you expect a chemical reaction to produce 4.38 dm3 of oxygen, O2, at 19oC and 101 kPa, what will be the volume at 25oC and 101 kPa?
A balloon contains 5.41 dm3 of helium, He, at 24oC and 101.5 kPa. Suppose the gas in the balloon is heated to 35oC. If the helium pressure is now 102.8 kPa, what is the volume of the gas?
Show that the moles of gas are proportional to the pressure for constant volume and temperature.
What is the pressure in a 50.0-L gas cylinder that contains 3.03 kg of oxygen, O2, at 23oC?
Calculate the density of helium, He, in grams per liter at 21oC and 752 mmHg. The density of air under these conditions is 1.188 g/L. What is the difference in mass between 1 liter of air and 1 liter
A sample of a gaseous substance at 25oC and 0.862 atm has a density of 2.26 g/L. What is the molecular mass of the substance?
How many liters of chlorine gas, Cl2, can be obtained at 40oC and 787 mmHg from 9.41 g of hydrogen chloride, HCl, according to the following equation? 2KMnO4(s) + 16HCl(aq) → 8H2O(l) + 2KCl(aq) +
Suppose that you set up two barometers like the one shown. In one of the barometers you use mercury, and in the other you use water. Which of the barometers would have a higher column of liquid, the
To conduct some experiments, a 10.0-L flask equipped with a movable plunger, as illustrated here, is filled with enough H2 gas to come to a pressure of 20 atm.a. In the first experiment, we decrease
Three 3.0-L flasks, each at a pressure of 878 mmHg, are in a room. The flasks contain He, Ar, and Xe, respectively. a. Which of the flasks contains the most atoms of gas? b. Which of the flasks has
A flask equipped with a valve contains 3.0 mol of H2 gas. You introduce 3.0 mol of Ar gas into the flask via the valve and then seal the flask. a. What happens to the pressure of just the H2 gas in
Consider the experimental apparatus shown. In this setup, each round flask contains a gas, and the long tube contains no gas (that is, it is a vacuum).a. We use 1.0 mol of He for experiment X and 1.0
A 1.00-L container is filled with an ideal gas and the recorded pressure is 350 atm.We then put the same amount of a real gas into the container and measure the pressure. a. If the real gas molecules
Define pressure. From the definition, obtain the SI unit of pressure in terms of SI base units.
A given volume of nitrogen, N2, required 68.3 s to effuse from a hole in a chamber. Under the same conditions, another gas required 85.6 s for the same volume to effuse. What is the molecular mass
Calculate the pressure of ethanol vapor, C2H5OH(g), at 82.0oC if 1.000 mol C2H5OH(g) occupies 30.00 L. Use the van der Waals equation (see Table 5.7 for data). Compare with the result from the ideal
Calculate the pressure of water vapor at 120.0oC if 1.000 mol of water vapor occupies 32.50 L. Use the van der Waals equation (see Table 5.7 for data). Compare with the result from the ideal gas law.
Calculate the molar volume of ethane at 1.00 atm and 0oC and at 10.0 atm and 0oC, using the van der Waals equation. The van der Waals constants are given in Table 5.7. To simplify, The term N2a/V2 is
Calculate the molar volume of oxygen at 1.00 atm and 0oC and at 10.0 atm and 0oC, using the van der Waals equation. The van der Waals constants are given in Table 5.7. (See the note on solving the
A glass tumbler containing 243 cm3 of air at 1.00 × 102 kPa (the barometric pressure) and 20oC is turned upside down and immersed in a body of water to a depth of 20.5 m. The air in the glass is
The density of air at 20oC and 1.00 atm is 1.205 g/L. If this air were compressed at the same temperature to equal the pressure at 40.0 m below sea level, what would be its density? Assume the
A flask contains 201 mL of argon at 21oC and 738 mmHg. What is the volume of gas, corrected to STP?
A steel bottle contains 12.0 L of a gas at 11.0 atm and 20oC. What is the volume of gas at STP?
A balloon containing 5.0 dm3 of gas at 14oC and 100.0 kPa rises to an altitude of 2000. m, where the temperature is 20oC. The pressure of gas in the balloon is now 79.0 kPa. What is the volume of gas
Starting from Boyles’s, Charles’s, and Avogadro’s laws, obtain the ideal gas law, PV = nRT.
A volume of air is taken from the earth’s surface, at 15oC and 1.00 atm, to the stratosphere, where the temperature is –21oC and the pressure is 1.00 × 10–3 atm. By what factor is the volume
A radioactive metal atom decays (goes to another kind of atom) by emitting an alpha particle (He2+ ion). The alpha particles are collected as helium gas. A sample of helium with a volume of 12.05 mL
The combustion method used to analyze for carbon and hydrogen can be adapted to give percentage N by collecting the nitrogen from combustion of the compound as N2. A sample of a compound weighing
Dry air at STP has a density of 1.2929 g/L. Calculate the average molecular weight of air from the density.
A hydrocarbon gas has a density of 1.22 g/L at 20oC and 1.00 atm. An analysis gives 80.0% C and 20.0% H. What is the molecular formula?
A person exhales about 5.8 × 102 L of carbon dioxide per day (at STP). The carbon dioxide exhaled by an astronaut is absorbed from the air of a space capsule by reaction with lithium hydroxide,
Pyruvic acid, HC3H3O3, is involved in cell metabolism. It can be assayed for (that is, the amount of it determined) by using a yeast enzyme. The enzyme makes the following reaction go to
Liquid oxygen was first prepared by heating potassium chlorate, KClO3, in a closed vessel to obtain oxygen at high pressure. The oxygen was cooled until it liquefied. 2KClO3(s) → 2KCl(s) +
Raoul Pictet, the Swiss physicist who first liquefied oxygen, attempted to liquefy hydrogen. He heated potassium formate, KCHO2, with KOH in a closed 2.50-L vessel. KCHO2(s) + KOH(s) → K2CO3(s) +
A 24.9-mL volume of hydrochloric acid reacts completely with 55.0 mL of aqueous Na2CO3. The reaction is 2HCl(aq) + Na2CO3(aq) → CO2(g) + H2O(l ) + 2NaCl(aq)
An 18.6-mL volume of hydrochloric acid reacts completely with a solid sample of MgCO3. The reaction is 2HCl(aq) + MgCO3(s) → CO2(g) + H2O(l ) + MgCl2(aq)
A 41.41-mL sample of a 0.1250 M acid reacts with an excess of Na2CO3 to form 150.0 mL CO2 at 646 mmHg and 27oC. If the acid is either HCl or H2SO4, which is it?
A 48.90-mL sample of a 0.2040 M acid reacts with an excess of Na2CO3 to form 125.0 mL CO2 at 722 mmHg and 17oC. If the acid is either HCl or H2SO4, which is it?
If the rms speed of NH3 molecules is found to be 0.605 km/s, what is the temperature (in degrees Celsius)?
If the rms speed of He atoms in the exosphere (highest region of the atmosphere) is 3.53 103 m/s, what is the temperature (in kelvins)?
Calculate the ratio of rates of effusion of 235UF6 and 238UF6, where 235U and 238U are isotopes of uranium. The atomic masses are 235U, 235.04 amu; 238U, 238.05 amu; 19F (the only naturally occurring
Hydrogen has two stable isotopes, 1H and 2H, with atomic masses of 1.0078 amu and 2.0141 amu, respectively. Ordinary hydrogen gas, H2, is a mixture consisting mostly of 1H2 and 1H2H. Calculate the
A 1.000-g sample of an unknown gas at 0oC gives the following data: P (atm) V (L)0.2500………………………….. 3.19080.5000…………………………..
Plot the data given in Table 5.3 for oxygen at 0oC to obtain an accurate molar mass for O2. To do this, calculate a value of the molar mass at each of the given pressures from the ideal gas law (we
Carbon monoxide, CO, and oxygen, O2, react according to2CO(g) + O2(g) 2CO2(g)Assuming that the reaction takes place and goes to completion, determine what substances remain and what
What is the value of R in units of L•mmHg/(K•mol)?
Suppose the apparatus shown in the figure accompanying Problem 5.129 contains H2 at 0.500 atm in the left vessel separated from O2 at 1.00 atm in the other vessel. The valve is then opened. If H2 and
How does nitrogen monoxide, NO, function in the body to regulate blood pressure?
Explain the greenhouse effect.
A 24.6-mL volume of a hydrochloric acid solution reacts completely with a solid sample of magnesium carbonate, producing 183 mL of CO2 that is collected over water at 24.0oC and 738 torr total
The graph below represents the distribution of molecular speeds of hydrogen and neon at 200 K.a. Match each curve to the appropriate gas. b. Calculate the rms speed (in m/s) for each of the gases at
A submersible balloon is sent to the bottom of the ocean. On shore, the balloon had a capacity of 162 L when it was filled at 21.0oC and standard pressure. When it reaches the ocean floor, which is
Showing 2500 - 2600
of 4002
First
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
Last