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general chemistry principles

Questions and Answers of General Chemistry Principles

A particular coal sample contains 3.28% S by mass. When the coal is burned, the sulfur is converted to SO2(g). What volume of SO2(g), measured at 23 °C and 738 mmHg, is produced by burning 1.2 x 106
What volume of O2(g) is consumed in the combustion of 75.6 L C3H8(g) if both gases are measured at STP?
A 3.57 g sample of a KCl–KClO3 mixture is decomposed by heating and produces 119 mL O2(g), measured at 22.4 °C and 98.3 kPa. What is the mass percent of KClO3 in the mixture? 2 KCIO3(s) 2 KCl(s) +
Hydrogen peroxide, H2O2, is used to disinfect contact lenses. How many milliliters of O2(g) at 22 °C and 1.00 bar can be liberated from 10.0 mL of an aqueous solution containing 3.00% H2O2 by mass?
Calculate the volume of H2(g), measured at 26 °C and 751 Torr, required to react with 28.5 L CO(g), measured at 0 °C and 760 Torr, in this reaction. 3 CO(g) + 7 H₂(g) C3H8(g) + 3 H₂O(1)
Which actions would you take to establish a pressure of 2.00 atm in a 2.24 L cylinder containing 1.60 g O2(g) at 0 °C? (a) Add 1.60 g O2;(b) Release 0.80 g O2;(c) Add 2.00 g He; (d) Add 0.60 g He.
A 2.00 L container is filled with Ar(g) at 752 mmHg and 35 °C. A 0.728 g sample of C6H6 vapor is then added.(a) What is the total pressure in the container?(b) What is the partial pressure of Ar and
A mixture of 4.0 g H2(g) and 10.0 g He(g) in a 5.2 L flask is maintained at 0 °C. (a) What is the total pressure in the container?(b) What is the partial pressure of each gas?
In the drawing below, 1.00 g H2(g) is maintained at 1 atm pressure in a cylinder closed off by a freely moving piston. Which sketch, (a), (b), or (c), best represents the mixture obtained when 1.00 g
The chemical composition of air that is exhaled (expired) is different from ordinary air. Atypical analysis of expired air at 37 °C and 1.00 atm, expressed as percent by volume, is 74.2% N2, 15.2%
A 4.0 L sample of O2 gas has a pressure of 1.0 bar. A 2.0 L sample of N2 gas has a pressure of 2.0 bar. If these two samples are mixed and then compressed in a 2.0 L vessel, what is the final
A 1.65 g sample of Al reacts with excess HCl, and the liberated H2 is collected over water at 25 °C at a barometric pressure of 744 mmHg. What volume of gaseous mixture, in liters, is collected? 2
The following figure shows the contents and pressures of three vessels of gas that are joined by a connecting tube.After the valves on the vessels are opened, the final pressure is measured and found
A sample of O2(g) is collected over water at 24 °C. The volume of gas is 1.16 L. In a subsequent experiment, it is determined that the mass of O2 present is 1.46 g. What must have been the
An 89.3 mL sample of wet O2(g) is collected over water at 21.3 °C at a barometric pressure of 756 mmHg (vapor pressure of water at 21.3 °C = 19 mmHg).(a) What is the partial pressure of O2(g) in
A 1.072 g sample of He(g) is found to occupy a volume of 8.446 L when collected over hexane at 25.0 °C and 738.6 mmHg barometric pressure. Use these data to determine the vapor pressure of hexane at
At elevated temperatures, solid sodium chlorate (NaClO3) decomposes to produce sodium chloride, NaCl, and O2 gas. A 0.8765 g sample of impure sodium chlorate was heated until the production of oxygen
When solid KClO3 is heated strongly, it decomposes to form solid potassium chloride, KCl, and O2 gas. A 0.415 g sample of impure KClO3 is heated strongly and the O2 gas produced by the decomposition
Calculate urms, in meters per second, for Cl2(g) molecules at 30 °C.
The urms of H2 molecules at 273 K is 1.84 x 103 m/s. At what temperature is urms for H2 twice this value?
Refer to Example 6-14. What must be the molecular mass of a gas if its molecules are to have a root-mean-square speed at 25 °C equal to the speed of the M-16 rifle bullet?Example 6-14Which is the
Refer to Example 6-14. Noble gases (group 18) exist as atoms, not molecules (they are monatomic). Cite one noble gas whose urms at 25 °C is higher than the speed of the rifle bullet and one whose
At what temperature will urms for Ne(g) be the same as urms for He at 300 K?
Determine um, u̅, and urms for a group of ten automobiles clocked by radar at speeds of 38, 44, 45, 48, 50, 55, 55, 57, 58, and 60 mi/h, respectively.
Calculate the average kinetic energy, E̅k for O2(g) at 298 K and 1.00 atm.
Calculate the total kinetic energy, in joules, of 155 g N2(g) at 25 °C and 1.00 atm.
If 0.00484 mol N2O(g) effuses through an orifice in a certain period of time, how much NO2(g) would effuse in the same time under the same conditions?
A sample of N2(g) effuses through a tiny hole in 38 s. What must be the molar mass of a gas that requires 64 s to effuse under identical conditions?
What are the ratios of the diffusion rates for the pairs of gases (a) N2 and O2;(b) H2O and D2O (D = deuterium, i.e., 12H); (c) 14CO2 and 12CO2;(d) 235UF6 and 238UF6?
Which of the following visualizations best represents the distribution of O2 and SO2 molecules near an orifice some time after effusion occurs in the direction indicated by the arrows? The initial
It takes 22 hours for a neon-filled balloon to shrink to half its original volume at STP. If the same balloon had been filled with helium, then how long would it have taken for the balloon to shrink
The molar mass of radon gas was first estimated by comparing its diffusion rate with that of mercury vapor, Hg(g). What is the molar mass of radon if mercury vapor diffuses 1.082 times as fast as
Use both the ideal gas equation and the van der Waals equation to calculate the pressure exerted by 1.50 mol of SO2(g) when it is confined at 298 K to a volume of (a) 100.0 L; (b) 50.0 L; (c) 20.0
Use the value of the van der Waals constant b for He(g) given in Table 6.5, to estimate the radius, r, of a single helium atom. Give your answer in picometers.Table 6.5 TABLE 6.5 van der Waals
Refer to Example 6-17. Recalculate the pressure of Cl2(g) by using both the ideal gas equation and the van der Waals equation at the temperatures (a) 100 °C;(b) 200 °C;(c) 400 °C.From the
(a) Use the value of the van der Waals constant b for CH4(g), given in Table 6.5, to estimate the radius of the CH4 molecule. (See Exercise 89.) How does your estimate of the radius compare with the
Assume the following initial conditions for the graphs labeled A, B, and C in Figure 6-7. (A) 10.0 mL at 400 K;(B) 20.0 mL at 400 K; (C) 40.0 mL at 400 K. Use Charles’s law to calculate the
Explain why it is necessary to include the density of Hg(l) and the value of the acceleration due to gravity, g, in a precise definition of a millimeter of mercury.
Consider the diagram to the right. The “initial” sketch illustrates, both at the macroscopic and molecular levels, an initial condition: 1 mol of a gas at 273 K and 1.00 bar. With as much detail
Two evacuated bulbs of equal volume are connected by a tube of negligible volume. One of the bulbs is placed in a constant-temperature bath at 225 K and the other bulb is placed in a
A compound is 85.6% carbon by mass. The rest is hydrogen. When 10.0 g of the compound is evaporated at 50.0 °C, the vapor occupies 6.30 L at 1.00 atm pressure. What is the molecular formula of the
A 3.05 g sample of NH4NO3(s) is introduced into an evacuated 2.18 L flask and then heated to 250 °C. What is the total gas pressure, in atmospheres, in the flask at 250 °C when the NH4NO3 has
Ammonium nitrite, NH4NO2, decomposes according to the chemical equation below.What is the total volume of products obtained when 128 g NH4NO2 decomposes at 819 °C and 101 kPa? NH4NO₂ (s)- N2(g) +
A 0.7178 g sample of a hydrocarbon occupies a volume of 390.7 mL at 65.0 C and 99.2 kPa. When the sample is burned in excess oxygen, 2.4267 g CO2 and 0.4967 g H2O are obtained. What is the molecular
A mixture of 1.00 g H2 and 8.60 g O2 is introduced into a 1.500 L flask at 25 °C. When the mixture is ignited, an explosive reaction occurs in which water is the only product. What is the total gas
In the reaction of CO2(g) and solid sodium peroxide (Na2O2), solid sodium carbonate (Na2CO3) and oxygen gas are formed. This reaction is used in submarines and space vehicles to remove expired CO2(g)
What is the partial pressure of Cl2(g), in millimeters of mercury, at 0.00 °C and 1.00 atm in a gaseous mixture that consists of 46.5% N2, 12.7% Ne, and 40.8% Cl2, by mass?
When working with a mixture of gases, it is sometimes convenient to use an apparent molar mass (a weighted average molar mass). Think in terms of replacing the mixture with a hypothetical single gas.
A gaseous mixture of He and O2 has a density of 0.518 g/L at 25 °C and 721 mmHg. What is the mass percent He in the mixture?
A mixture of N2O(g) and O2(g) can be used as an anesthetic. In a particular mixture, the partial pressures of N2O and O2 are 612 Torr and 154 Torr, respectively.Calculate (a) The mass percentage of
The accompanying sketch is that of a closed-end manometer. Describe how the gas pressure is measured. Why is a measurement of Pbar. not necessary when using this manometer? Explain why the closed-end
Gas cylinder A has a volume of 48.2 L and contains N2(g) at 8.35 atm at 25 °C. Gas cylinder B, of unknown volume, contains He(g) at 9.50 atm and 25 °C. When the two cylinders are connected and the
Producer gas is a type of fuel gas made by passing air or steam through a bed of hot coal or coke. Atypical producer gas has the following composition in percent by volume: 8.0% CO2, 23.2% CO, 17.7%
The amount of ozone, O3, in a mixture of gases can be determined by passing the mixture through a solution of excess potassium iodide, KI. Ozone reacts with the iodide ion as follows:The amount of
Chlorine dioxide, ClO2, is sometimes used as a chlorinating agent for water treatment. It can be prepared from the reaction below:In an experiment, 1.0 L Cl2(g) measured at 10.0 °C and 4.66 atm, is
A mixture of H2(g) and O2(g) is prepared by electrolyzing 1.32 g water, and the mixture of gases is collected over water at 30 °C and 748 mmHg. The volume of “wet” gas obtained is 2.90 L. What
What volume of air, measured at 298 K and 101 kPa, is required to burn 2.00 kg C8H18? Air is approximately 78.1% N2 and 20.9% O2, by volume. Other gases make up the remaining 1.0%.
Aluminum (Al) and iron (Fe) each react with hydrochloric acid solution (HCl) to produce a chloride salt and hydrogen gas, H2(g). A 0.1924 g sample of a mixture of Al and Fe is treated with excess HCl
A 0.168 L sample of O2(g) is collected over water at 26 °C and a barometric pressure of 737 mmHg. In the gas that is collected, what is the percent water vapor (a) By volume; (b) By number of
A 0.1052 g sample of in an 8.050 L sample of H2O(l) dry air at 30.1 °C evaporates completely. To what temperature must the air be cooled to give a relative humidity of 80.0%? Vapor pressures of
A breathing mixture is prepared in which He is substituted for N2. The gas is 79% He and 21% O2, by volume. (a) What is the density of this mixture in grams per liter at 25 °C and 1.00 atm? (b) At
An alternative to Figure 6-6 is to plot P against 1/V. The resulting graph is a straight line passing through the origin. Use Boyle’s data from Feature Problem 125 to draw such a straight-line
We have noted that atmospheric pressure depends on altitude. Atmospheric pressure as a function of altitude can be calculated with an equation known as the barometric formula:In this equation, P and
Consider a sample of O2(g) at 298 K and 1.0 atm. Calculate (a) urms and (b) The fraction of molecules that have speed equal to urms.
A nitrogen molecule (N2) having the average kinetic energy at 300 K is released from Earth’s surface to travel upward. If the molecule could move upward without colliding with other molecules, then
For at and 1 atm, calculate the percentage of molecules that have speed (a) 0 m s-1;(b) 500 m s-1;(c) 1000 m s-1;(d) 1500 m s-1;(e) 2000 m s-1;(f) 2500 m s-1;(g) 3500 m s-1.Graph your results to
If the van der Waals equation is solved for volume, a cubic equation is obtained.(a) Derive the equation below by rearranging equation (6.26).(b) What is the volume, in liters, occupied by 185 g
According to the CRC Handbook of Chemistry and Physics (95th ed.), the molar volume of O2(g) is 0.2168 L mol-1 at 280 K and 10 MPa.(a) Use the van der Waals equation to calculate the pressure of one
A particular equation of state for O2(g) has the formwhere V̅ is the molar volume, B = -21.89 cm3/mol and C = 1230 cm6/mol2. (a) Use the equation to calculate the pressure exerted by 1 mol O2(g)
Shown below is a diagram of Boyle’s original apparatus. At the start of the experiment, the length of theair column (A) on the left was 30.5 cm and the heights of mercury in the arms of the tube
A 0.156 g sample of a magnesium–aluminum alloy dissolves completely in an excess of HCl(aq). The liberated H2(g) is collected over water at 5 °C when the barometric pressure is 752 Torr. After the
The equation d/P = M/RT, which can be derived from equation (6.14), suggests that the ratio of the density (d) to pressure (P) of a gas at constant temperature should be a constant. The gas density
In research that required the careful measurement of gas densities, John Rayleigh, a physicist, found that the density of O2(g) had the same value whether the gas was obtained from air or derived
A sounding balloon is a rubber bag filled with H2(g) and carrying a set of instruments (the payload). Because this combination of bag, gas, and payload has a smaller mass than a corresponding volume
In your own words, define or explain each term or symbol. (a) Atm; (b) STP; (c) R; (d) Partial pressure;(e) urms.
Briefly describe each concept or process: (a) Absolute zero of temperature; (b) Collection of a gas over water; (c) Effusion of a gas; (d) Law of combining volumes.
Explain the important distinctions between(a) Barometer and manometer; (b) Celsius and Kelvin temperature; (c) Ideal gas equation and general gas equation; (d) Ideal gas and real gas.
Which exerts the greatest pressure, (a) A 75.0 cm column of Hg(l) (d = 13.6 g/mL);(b) A column of air 10 mi high; (c) A 5.0 m column of CCl4(l) (d = 1.59 g/mL);(d) 10.0 g H2(g) at STP?
For a fixed amount of gas at a fixed pressure, changing the temperature from 100.0 °C to 200 K causes the gas volume to (a) Double; (b) Increase, but not to twice its original value; (c)
Two gases were mixed into a 5.000 L container at 291.0 K. Gas Awas originally confined in 14.20 L at 1.081 bar and 303.1 K. Gas B was originally confined in 1.251 L at 26.77 bar and 327.5 K.(a) What
A fragile glass vessel will break if the internal pressure equals or exceeds 2.0 bar. If the vessel is sealed at 0 °C and 1.0 bar, then at what temperature will the vessel break? Assume that the
Which of the following choices represents the molar volume of an ideal gas at and 1.5 atm?(a) (298 x 1.5/273) x 22.4 L;(b) 22.4 L;(c) (273 x 1.5/298) x 22.4 L;(d) [298/(273 x 1.5)] x 22.4 L;(e)
The gas with the greatest density at STP is (a) N2O;(b) Kr; (c) SO3;(d) Cl2.
Precisely 1 mol of helium and 1 mol of neon are mixed in a container. (a) Which gas has the greater average molecular speed? (b) Which type of molecule strikes the wall of the container more
If the Kelvin temperature of a gas doubles, then which of the following also doubles? (a) The average molecular speed;(b) The speed of every molecule;(c) The kinetic energy of every molecule; (d)
The postulates of the kinetic molecular theory of gases include all those that follow except (a) No forces exist between molecules; (b) Molecules are point masses; (c) Molecules are repelled by
A sample of O2(g) is collected over water at 23 °C and a barometric pressure of 751 Torr. The vapor pressure of water at 23 °C is 21 mmHg. The partial pressure of O2(g) in the sample collected
At 0 °C and 0.500 atm, 4.48 L of gaseous NH3(a) Contains 6.02 x 1022 molecules; (b) Has a mass of 17.0 g;(c) Contains 0.200 mol NH3; (d) Has a mass of 3.40 g.
Carbon monoxide, CO, and hydrogen react according to the equation below.What volume of which reactant gas remains if 12.0 L CO(g) and 25.0 L H2(g) are allowed to react? Assume that the volumes of
To establish a pressure of 2.00 atm in a 2.24 L cylinder containing 1.60 g O2(g) at 0 °C,(a) Add 1.60 g O2;(b) Add 0.60 g He(g);(c) Add 2.00 g He(g);(d) Release 0.80 g O2(g).
A mixture of 5.0 x 10-5 mol H2(g) and 5.0 x 10-5 mol SO2(g) is placed in a 10.0 L container at 25 °C. The container has a pinhole leak. After a period of time, the partial pressure of H2(g) in the
Under which conditions is Cl2 most likely to behave like an ideal gas? Explain. (a) 100 °C and 10.0 atm;(b) 0 °C and 0.50 atm; (c) 200 °C and 0.50 atm;(d) 400 °C and 10.0 atm.
Without referring to Table 6.5, state which species in each of the following pairs has the greater value for the van der Waals constant a, and which one has the greater value for the van der Waals
Explain why the height of the mercury column in a barometer is independent of the diameter of the barometer tube.
A gaseous hydrocarbon that is 82.7% C and 17.3% H by mass has a density of 2.35 g/L at 25 °C and 752 Torr. What is the molecular formula of this hydrocarbon?
In 1860, Stanislao Cannizzaro showed how Avogadro’s hypothesis could be used to establish the atomic masses of elements in gaseous compounds. Cannizzaro took the atomic mass of hydrogen to be
Phosphorus forms two compounds with chlorine. In the first compound, 1.000 g of phosphorus is combined with 3.433 g chlorine, and in the second, 2.500 g phosphorus is combined with 14.308 g chlorine.
In the sample of sulfur weighing 4.07 g pictured in Figure 2-18, (a) How many moles of sulfur are present, and(b) What is the total number of sulfur atoms in the sample?Figure 2-18 RECCUBERK200
(A) How many Pb atoms are present in a small piece of lead with a volume of 0.105 cm3? The density of Pb = 11.34 g/cm3.(B) Rhenium-187 is a radioactive isotope that can be used to determine the age
In one experiment, 2.18 g sodium was allowed to react with 16.12 g chlorine. All the sodium was used up, and 5.54 g sodium chloride (salt) was produced. In a second experiment, 2.10 g chlorine was

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