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chemistry
physical chemistry

Questions and Answers of Physical Chemistry

Hydrogen cyanide gas is commercially prepared by the reaction of methane [CH4(g)], ammonia [NH3(g)], and oxygen [O2(g)] at a high temperature. The other product is gaseous water.a. Write a balanced
A sealed balloon is filled with 1.00 L of helium at 23oC and 1.00 atm. The balloon rises to a point in the atmosphere where the pressure is 220. torr and the temperature is 231oC. What is the change
Consider a children’s cartoon illustrating a child holding the strings of several helium balloons and being lifted into the sky.a. Estimate the minimum number of 10-L balloons it would take to lift
A 16.0-g sample of methane (CH4) reacts with 64.0 g of oxygen gas in a container fitted with a piston (at 1.00 atm and 425 K). Methane can react with oxygen to form carbon dioxide and water vapor or
You have two samples of helium gas at the same pressure in separate steel containers of the same volume. You want the number of collisions of helium atoms with the walls of container 1 to be twice
A mixture of chromium and zinc weighing 0.362 g was reacted with an excess of hydrochloric acid. After all the metals in the mixture reacted, 225 mL of dry hydrogen gas was collected at 27oC and 750.
You have a sealed, flexible balloon filled with argon gas. The atmospheric pressure is 1.00 atm and the temperature is 25oC. The air has a mole fraction of nitrogen of 0.79, the rest being oxygen.a.
Derive a linear relationship between gas density and tem-perature, and use it to estimate the value of absolute zero temperature (in oC to the nearest 0.1oC) from an air sample whose density is
A chemist weighed out 5.14 g of a mixture containing unknown amounts of BaO(s) and CaO(s) and placed the sample in a 1.50-L flask containing CO2(g) at 30.0oC and 750. torr. After the reaction to form
The density of a pure gaseous compound was measured at 0.00oC as a function of pressure to give the following results:Density (g/ L) …………………………. Pressure (atm)0.17893
Consider separate 1.0-L samples of He(g) and UF6(g), both at 1.00 atm and containing the same number of moles. What ratio of temperatures for the two samples would produce the same collision
The most probable velocity ump is the velocity possessed by the greatest number of gas particles. At a certain temperature, the probability that a gas particle has the most probable velocity is equal
A piece of solid carbon dioxide, with a mass of 22.0 g, is placed in an otherwise empty 4.00-L container at 278C. What is the pressure in the container after all the carbon dioxide vaporizes? If 22.0
Derive Dalton’s law of partial pressures from the kinetic molecular theory of gases. What assumptions are necessary?
One of the assumptions of the kinetic molecular theory is that the volume of a gas particle is negligible. If this were the case, the ratio of the number of collisions of gas particles with the walls
Consider a sample of a hydrocarbon (a compound con-sisting of only carbon and hydrogen) at 0.959 atm and 298 K. Upon combusting the entire sample in oxygen, you collect a mixture of gaseous carbon
A steel cylinder contains 5.00 moles of graphite (pure carbon) and 5.00 moles of O2. The mixture is ignited and all the graphite reacts. Combustion produces a mixture of CO gas and CO2 gas. After the
You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/ L. Assume ideal behavior and constant
Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/ min at 1.50 atm and ambient temperature. Air is added to the chamber at 1.00 atm and the same temperature, and the gases are
A spherical vessel with a volume of 1.00 L was evacuated and sealed. Twenty- four hours later the pressure of air in the vessel was found to be 1.20 × 10-6 atm. During this 24-h period, the vessel
Calculate the number of stages needed to change a mixture of 13CO2 and 12CO2 that is originally 0.10% (by moles) 13CO2 to a mixture that is 0.010% 13CO2 by a gaseous diffusion process. (The mass of
Two samples of gas are separated in two rectangular 1.00-L chambers by a thin metal wall. One sample is pure helium and the other is pure radon. Both samples are at 27°C and show a pressure of 2.00
You have a helium balloon at 1.00 atm and 25oC. You want to make a hot-air balloon with the same volume and same lift as the helium balloon. Assume air is 79.0% nitrogen and 21.0% oxygen by volume.
An ideal gas is in a cylinder with a volume of 5.0 × 102 mL at a temperature of 30.oC and a pressure of 710 torr. The gas is compressed to a volume of 25 mL, and the temperature is raised to 820oC.
Consider an equimolar mixture (equal number of moles) of two diatomic gases (A2 and B2) in a container fitted with a piston. The gases react to form one product (which is also a gas) with the formula
You are given an unknown gaseous binary compound (that is, a compound consisting of two different elements). When 10.0 g of the compound is burned in excess oxygen, 16.3 g of water is produced. The
Use the following information to identify element A and compound B, then answer questions a and b. An empty glass container has a mass of 658.572 g. It has a mass of 659.452 g after it has been
Suppose two 200.0- L tanks are to be filled separately with the gases helium and hydrogen. What mass of each gas is needed to produce a pressure of 135 atm in its respective tank at 24oC?
An ideal gas at 7oC is in a spherical flexible container having a radius of 1.00 cm. The gas is heated at constant pressure to 88oC. Determine the radius of the spherical container after the gas is
A flask that can withstand an internal pressure of 2500 torr, but no more, is filled with a gas at 21.0oC and 758 torr and heated. At what temperature will it burst?
A gas sample containing 1.50 moles at 25oC exerts a pressure of 400. torr. Some gas is added to the same container, and the temperature is increased to 50oC. If the pressure increases to 800. torr,
Consider the following chemical equation:2NO2(g) → N2O4(g)If 25.0 mL of NO2 gas is completely converted to N2O4 gas under the same conditions, what volume will the N2O4 occupy?
A bicycle tire is filled with air to a pressure of 75 psi at a temperature of 19oC. Riding the bike on asphalt on a hot day increases the temperature of the tire to 58oC. The volume of the tire
A diagram for an open- tube manometer is shown below. If the flask is open to the atmosphere, the mercury levels are equal. For each of the following situations in which a gas is contained in
A hot-air balloon is filled with air to a volume of 4.00 × 103 m3 at 745 torr and 21oC. The air in the balloon is then heated to 62oC, causing the balloon to expand to a volume of 4.20 × 103 m3.
Determine the partial pressure of each gas as shown in the figure below. The relative numbers of each type of gas are depicted in the figure.
Consider the flasks in the following diagrams.a. Which is greater, the initial pressure of helium or initial pressure of neon? How much greater?b. Assuming the connecting tube has negligible volume,
A sample of nitrogen gas was collected over water at 20.oC and a total pressure of 1.00 atm. A total volume of 2.50 × 102 mL was collected. What mass of nitrogen was collected? (At 20.oC the vapor
Helium is collected over water at 25oC and 1.00 atm total pressure. What total volume of gas must be collected to obtain 0.586 g of helium? (At 25oC the vapor pressure of water is 23.8 torr.)
A 2.00- L sample of O2(g) was collected over water at a total pressure of 785 torr and 25oC. When the O2(g) was dried (water vapor removed), the gas had a volume of 1.94 L at 25oC and 785 torr.
In a mixture of the two gases, the partial pressures of CH4(g) and O2(g) are 0.175 atm and 0.250 atm, respectively.a. What is the mole fraction of each gas in the mixture?b. If the mixture occupies a
A 1.00- L gas sample at 100oC and 600. torr contains 50.0% helium and 50.0% xenon by mass. What are the partial pressures of the individual gases?
At 0oC a 1.0 L flask contains 5.0 × 10-2 mole of N2, 1.5 × 102 mg O2, and 5.0 × 10-1 molecules of NH3. What is the partial pressure of each gas, and what is the total pressure in the flask?
Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 78% N2, 21% O2, and 1.0% Ar, what is the density of air at standard temperature and pressure?
The gravitational force exerted by an object is given by F = mg where F is the force in newtons, m is the mass in kilograms, and g is the acceleration due to gravity, 9.81 m/ s2. Calculate the force
Consider two different containers, each filled with 2 moles of Ne(g). One of the containers is rigid and has constant volume. The other container is flexible (like a balloon) and is capable of
An unknown diatomic gas has a density of 3.164 g/ L at STP. What is the identity of the gas?
A compound contains only nitrogen and hydrogen and is 87.4% nitrogen by mass. A gaseous sample of the com-pound has a density of 0.977 g/ L at 710. torr and 100oC. What is the molecular formula of
A compound has the empirical formula CHCl. A 256-mL flask, at 373 K and 750. torr, contains 0.800 g of the gaseous compound. Give the molecular formula.
One of the chemical controversies of the nineteenth century concerned the element beryllium (Be). Berzelius originally claimed that beryllium was a trivalent element (forming Be3+ ions) and that it
Discrepancies in the experimental values of the molar mass of nitrogen provided some of the first evidence for the existence of the noble gases. If pure nitrogen is collected from the decomposition
A sample of methane (CH4) gas contains a small amount of helium. Calculate the volume percentage of helium if the density of the sample is 0.70902 g/ L at 0.0oC and 1.000 atm.
Metallic molybdenum can be produced from the mineral molybdenite (MoS2). The mineral is first oxidized in air to molybdenum trioxide and sulfur dioxide. Molybde-num trioxide is then reduced to
In 1897 the Swedish explorer Andreé tried to reach the North Pole in a balloon. The balloon was filled with hydrogen gas. The hydrogen gas was prepared from iron splints and diluted sulfuric acid.
Urea (H2NCONH2) is used extensively as a nitrogen source in fertilizers. It is produced commercially from the reaction of ammonia and carbon dioxide:Ammonia gas at 223oC and 90. atm flows into a
a. If the open-tube manometer in Exercise 22 contains a nonvolatile silicone oil (density = 1.30 g/cm3) instead of mercury (density = 13.6 g/ cm3), what are the pressures in the flask as shown in
Methanol (CH3OH) can be produced by the following reaction:CO(g) + 2H2(g) → CH3OH(g)Hydrogen at STP flows into a reactor at a rate of 16.0 L/min. Carbon monoxide at STP flows into the re-actor at a
Consider the reaction between 50.0 mL of liquid methanol (CH3OH; density = 0.850 g/ mL) and 22.8 L of O2 at 27oC and a pressure of 2.00 atm. The products of the reaction are CO2(g) and H2O(g).
Some very effective rocket fuels are composed of light-weight liquids. The fuel composed of dimethylhydrazine [(CH3) 2N2H2] mixed with dinitrogen tetroxide was used to power the lunar lander in its
Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This action causes sodium azide (NaN3) to decompose explosively according
At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The
Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400oC in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine
The nitrogen content of organic compounds can be determined by the Dumas method. The compound in question is first reacted by passage over hot CuO(s):The gaseous products are then passed through a
An organic compound contains C, H, N, and O. Combustion of 0.1023 g of the compound in excess oxygen yielded 0.2766 g of CO2 and 0.0991 g of H2O. A sample of 0.4831 g of the compound was analyzed for
Nitric acid is produced commercially by the Ostwald process. In the first step, ammonia is oxidized to nitric oxide:4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)Assume this reaction is carried out in the
Consider the following balanced equation in which gas X forms gas X2: 2X(g) → X2(g) Equal moles of X are placed in two separate containers. One container is rigid, so the volume cannot change; the
Freon-12 (CF2Cl2) is commonly used as the refrigerant in central home air conditioners. The system is initially charged to a pressure of 4.8 atm. Express this pressure in each of the following units
As NH3(g) is decomposed into nitrogen gas and hydrogen gas at constant pressure and temperature, the volume of the product gases collected is twice the volume of NH3 reacted. Explain. As NH3(g) is
Use the postulates of the kinetic molecular theory (KMT) to explain why Boyle’s law, Charles’s law, Avogadro’s law, and Dalton’s law of partial pressures hold true for ideal gases. Use the
You have a gas in a container fitted with a piston and you change one of the conditions of the gas such that a change takes place, as shown below:State two distinct changes you can make to accomplish
You have a gas in a container fitted with a piston and you change one of the conditions of the gas such that a change takes place, as shown below:
Consider two gases, A and B, each in a 1.0- L container with both gases at the same temperature and pressure. The mass of gas A in the container is 0.34 g, and the mass of gas B in the container is
Consider the following samples of gases at the same temperature.Arrange each of these samples in order from lowest to highest.a. Pressureb. Average kinetic energyc. Densityd. Root mean square
Calculate the average kinetic energies of the CH4 and N2 molecules at 273 K and 546 K.
Calculate the root mean square velocities of CH4 and N2 molecules at 273 K and 546 K.
Do all the molecules in a 1-mole sample of CH4(g) have the same kinetic energy at 273 K? Do all the molecules in a 1-mole sample of N2(g) have the same velocity at 546 K? Explain.
Consider separate 1.0- L gaseous samples of H2, Xe, Cl2, and O2, all at STP.a. Rank the gases in order of increasing average kinetic energy.b. Rank the gases in order of increasing average
Draw a qualitative graph to show how the first property varies with the second in each of the following (assume 1 mole of an ideal gas and T in kelvins).a. PV versus V with constant Tb. P versus T
Consider three identical flasks filled with different gases. Flask A: CO at 760 torr and 0oC Flask B: N2 at 250 torr and 0oC Flask C: H2 at 100 torr and 0oCa. In which flask will the molecules have
Consider a 1.0- L container of neon gas at STP. Will the average kinetic energy, root mean square velocity, frequency of collisions of gas molecules with each other, frequency of collisions of gas
Freon-12 is used as a refrigerant in central home air conditioners. The rate of effusion of Freon- 12 to Freon- 11 (molar mass = 137.4 g/ mol) is 1.07: 1. The formula of Freon-12 is one of the
One way of separating oxygen isotopes is by gaseous dif-fusion of carbon monoxide. The gaseous diffusion process behaves like an effusion process. Calculate the relative rates of effusion of 12C16O,
The rate of effusion of a particular gas was measured to be 24.0 mL/ min. Under the same conditions, the rate of effusion of pure methane gas (CH4) is 47.8 mL/ min. What is the molar mass of the
It took 4.5 minutes for 1.0 L of helium to effuse through a porous barrier. How long will it take for 1.0 L of Cl2 gas to effuse under identical conditions?
Calculate the pressure exerted by 0.5000 mole of N2 in a 1.0000-L container at 25.0oC. (See Table)a. Use the ideal gas law.b. Use the van der Waals equation.c. Compare the results from parts a and
Calculate the pressure exerted by 0.5000 mole of N2 in a 10.000- L container at 25.0oC. (See Table)a. Use the ideal gas law.b. Use the van der Waals equation.c. Compare the results from parts a and
Why do real gases not always behave ideally? Under what conditions does a real gas behave most ideally? Why?
Consider the following velocity distribution curves A and B.a. If the plots represent the velocity distribution of 1.0 L of He(g) at STP versus 1.0 L of Cl2(g) at STP, which plot corresponds to each
Consider the flasks in the following diagrams.Assuming the connecting tube has negligible volume, draw what each diagram will look like after the stopcock between the two flasks is opened. Also,
In the van der Waals equation, why is a term added to the observed pressure and why is a term subtracted from the container volume to correct for nonideal gas behavior?
From the values in Table for the van der Waals constant a for the gases H2, CO2, N2, and CH4, predict which molecule shows the strongest intermolecular attractions.Table
The Maxwell–Boltzmann distribution function f(u) increases at small values of u and decreases at large values of u. Identify the parts of the function responsible for this behavior.
Calculate the root mean square, the most probable, and the average velocities for N2(g) at 227°C.
Calculate the kinetic energy possessed by 1.00 × 1020 molecules of methane gas (CH4) at T = 27oC, assuming ideal behavior.
A flask contains 13 mole of H2 and 23 mole of He. Compare the force on the wall per impact of H2 relative to that for He.
A certain sample of uranium is reacted with fluorine to form a mixture of 235UF6(g) and 238UF6(g). After 100 diffusion steps, the gas contains 1526 235UF6 molecules per 1.000 × 105 total number of
Consider separate 1.0-L samples of O2(g) and He(g), both at 25°C and the same pressure. Compare the change in momentum per impact and the number of impacts per second in the two samples.
Consider separate 1.00-L samples of Ar(g), both containing the same number of moles, one at 27oC and the other at 77oC. Compare the change in momentum per impact and the number of impacts per second
Calculate the intermolecular collision frequency and the mean free path in a sample of helium gas with a volume of 5.0 L at 27oC and 3.0 atm. Assume that the diameter of a helium atom is 50 pm.
Consider the flask diagramed below. What are the final partial pressures of H2 and N2 after the stopcock between the two flasks is opened? (Assume the final volume is 3.00 L.) What is the total

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