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general chemistry principles
General Chemistry Principles And Modern Applications 11th Edition Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette - Solutions
(A) Suppose that the mercury level in Example 6-2 is 7.8 mm higher in the arm open to the atmosphere than in the closed arm. What would be the value of Pgas?(B) Suppose Pbar. and Pgas are those described in Example 6-2, but the manometer is filled with liquid glycerol (d = 1.26 g/cm3) instead of
Explain how the action of a water siphon is related to that of a suction pump.
When the manometer in Figure 6-5(c) is filled with liquid mercury (d = 13.6 g/cm3) the barometric pressure is 748.2 mmHg, and the difference in mercury levels is 8.6 mmHg. What is the gas pressure Pgas?Figure 6-5(c) Ph bar. n P h gas P gas 220 = Pbar + AP Gas (AP=-gxhxd
Calculate the height of a mercury column required to produce a pressure (a) Of 0.984 atm; (b) Of 928 Torr;(c) Equal to that of a column of water 142 ft high.
A 50.0 L cylinder contains nitrogen gas at a pressure of 21.5 atm. The contents of the cylinder are emptied into an evacuated tank of unknown volume. If the final pressure in the tank is 1.55 atm, then what is the volume of the tank?(a) (21.5/1.55) x 50.0 L;(b) (1.55/21.5) x 50.0 L;(c) 21.5/(1.55 x
(A) The 1.000 kg green cylinder in Figure 6-2 has a diameter of 2.60 cm. What pressure, expressed in Torr, does this cylinder exert on the surface beneath it?(B) We want to increase the pressure exerted by the 1.000 kg red cylinder in Example 6-3 to 100.0 mbar by placing a weight on top of it. What
Calculate the height of a column of liquid benzene (d = 0.879 g/cm3), in meters, required to exert a pressure of 0.970 atm.
The 1.000 kg red cylinder in Figure 6-2 has a diameter of 4.10 cm. What pressure, expressed in Torr, does this cylinder exert on the surface beneath it?Figure 6-2
A balloon is inflated to a volume of 2.50 L inside a house that is kept at 24 °C. Then it is taken outside on a very cold winter day. If the temperature outside is -25 °C, what will be the volume of the balloon when it is taken outside? Assume that the quantity of air in the balloon and its
Doubling a gas temperature from 100 K to 200 K causes a gas volume to double. Would you expect a similar doubling of the gas volume when a gas is heated from 100 °C to 200 °C? Explain.
(A) What is the volume occupied by 20.2 g NH3(g) at -25° C and 752 mmHg?(B) At what temperature will a 13.7 g Cl2 sample exert a pressure of 0.993 bar when confined in a 7.50 L container?
Calculate the height of a column of liquid glycerol (d = 1.26 g/cm3), in meters, required to exert the same pressure as 3.02 m of CCl4(l) (d = 1.59 g/cm3).
Would the answer in Example 6-10 be greater than, less than, or equal to 0.667 L if (a) Both gases were measured at STP; (b) If the O2 were measured at STP and the SO2 were measured at 25 °C and 98.0 kPa?Example 6-10Zinc blende, ZnS, is the most important zinc ore. Roasting (strong heating) of
What is the volume occupied by 13.7 g Cl2(g) at 45 °C and 98.4 kPa?
What is the pressure (in mmHg) of the gas inside the apparatus below if Pbar. = 740 mmHg, h1 = 30 mm, and h2 = 50 mm? Gas bar. I I I h₁ 1₂ Mercury (Hg)
(A) How many moles of He(g) are in a 5.00 L storage tank filled with helium at 10.5 atm pressure at 30.0 °C?(B) How many molecules of N2(g) remain in an ultrahigh vacuum chamber of 3.45 m3 volume when the pressure is reduced to 6.67 x 10-7 Pa at 25 °C?
Without doing a detailed calculation, state the outcome(s) you would expect in Figure 6-12(c) if an additional 0.50 mol H2 were added to the cylinder in Figure 6-12(a): (a) The mole fraction of H2 would double; (b) The partial pressure of He would remain the same; (c) The mole fraction of He
What is the pressure, in kilopascals, exerted by 1.00 x 1020 molecules of N2 in a 305 mL flask at 175 °C?
What is the pressure (in mmHg) of the gas inside the apparatus below if Pbar. = 740 mmHg, h1 = 30 mm, and h2 = 40 mm? Gas P bar. h₁ H Mercury (Hg) m₂
(A) A 1.00 mL sample of N2(g) at 36.2 °C and 2.14 atm is heated to 37.8 °C, and the pressure changed to 1.02 atm. What volume does the gas occupy at this final temperature and pressure?(B) Suppose that in Figure 6-10 we want the pressure to remain at 1.00 bar when the O2(g) is heated to 100 °C.
The situation pictured in Figure 6-10(a) is changed to that in Figure 6-10(b). What is the gas pressure in Figure 6-10(b)?Figure 6-10(a)Figure 6-10(b) To manometer 1.00 L O₂(g) at STP (a) Ice bath Thermometer
Without performing an actual calculation, indicate which has the greater urms, He(g) at 1000 K or H2(g) at 250 K.
(A) The same glass vessel used in Example 6-7 is filled with an unknown gas at 772 mmHg and 22.4 °C. The gas-filled vessel weighs 40.4868 g. What is the molar mass of the gas?(B) A 1.27 g sample of an oxide of nitrogen, believed to be either NO or N2O, occupies a volume of 1.07 L at 25 °C and
At times, a pressure is stated in units of mass per unit area rather than force per unit area. Express P = 1 atm in the unit kg/cm2.
Propylene is an important commercial chemical used in the synthesis of other organic chemicals and in production of plastics (polypropylene). A glass vessel weighs 40.1305 g when clean, dry, and evacuated; it weighs 138.2410 g when filled with water at 25.0 °C (density of water = 0.9970 g/mL) and
Which answer(s) is (are) true when comparing 1.0 mol at STP and 0.50 mol H2(g) He(g) at STP? The two gases have equal (a) Average molecular kinetic energies; (b) Root-mean-square speeds; (c) Masses; (d) Volumes; (e) Densities;(f) Effusion rates through the same orifice.
(A) What is the density of helium gas at 298 K and 0.987 bar? Based on your answer, explain why we can say that helium is “lighter than air.”(B) The density of a sample of gas is 1.00 g/L at 745 mmHg and 109 °C. What is the molar mass of the gas?
What is the density of oxygen gas (O2) at 298 K and 0.987 bar?
Following are the measured densities at 20.0 °C and 1 atm pressure of three gases: O2, 1.331 g/L; OF2, 2.26 g/L; NO, 1.249 g/L. Arrange them in the order of increasing adherence to the ideal gas equation.
(A) How many grams of NaN3 are needed to produce 20.0 L of N2(g) at 30.0 °C and 776 mmHg?(B) How many grams of Na(l) are produced per liter of N2(g) formed in the decomposition of sodium azide if the gas is collected at 25 °C and 1.00 bar?
What volume of N2, measured at 98.0 kPa and 26 °C, is produced when 75.0 g NaN3 is decomposed? 2 NaN3(s) 2 Na(1) + 3 N₂(g)
A sample of O2(g) has a volume of 26.7 L at 762 Torr. What is the new volume if, with the temperature and amount of gas held constant, the pressure is (a) Lowered to 385 Torr; (b) Increased to 3.68 atm?
(A) The first step in making nitric acid is to convert ammonia to nitrogen monoxide. This is done under conditions of high temperature and in the presence of a platinum catalyst. What volume of O2(g) is consumed per liter of NO(g) formed?(B) If all gases are measured at the same temperature and
Zinc blende, ZnS, is the most important zinc ore. Roasting (strong heating) of ZnS in oxygen is the first step in the commercial production of zinc.What volume of SO2(g) can be obtained from 1.00 L O2(g) and excess ZnS(s)? Both gases are measured at 25 °C and 98.0 kPa. 2 ZnS(s) + 30₂(g) 2 ZnO(s)
An 886 mL sample of Ne(g) is at 752 mmHg and 26 °C. What will be the new volume if, with the pressure and amount of gas held constant, the temperature is(a) Increased to 98 °C;(b) Lowered to -20 °C?
What is the pressure, in bar, exerted by a mixture of 1.0 g H2 and 5.00 g He when the mixture is confined to a volume of 5.0 L at 20 °C?
(A) What will be the total gas pressure, in bar, if 12.5 g Ne is added to the mixture of gases described in Example 6-11 and the temperature is then raised to 55 °C?(B) 2.0 L of O2(g) and 8.0 L of N2(g), each at 0.00 °C and 1.00 atm, are mixed together. The nonreactive gaseous mixture is
If 3.0 L of oxygen gas at 177 °C is cooled at constant pressure until the volume becomes 1.50 L, then what is the final temperature?
What are the partial pressures of H2 and He in the gaseous mixture described in Example 6-11?Example 6-11What is the pressure, in bar, exerted by a mixture of 1.0 g H2 and 5.00 g He when the mixture is confined to a volume of 5.0 L at 20 °C?
We want to change the volume of a fixed amount of gas from 725 mL to 2.25 L while holding the temperature constant. To what value must we change the pressure if the initial pressure is 105 kPa?
(A) A mixture of 0.197 mol CO2(g) and 0.00278 mol H2O(g) is held at 30.0 °C and 2.50 atm. What is the partial pressure of each gas?(B) The percent composition of air by volume is 78.08% N2, 20.95% O2, 0.93% Ar, and 0.036% CO2.What are the partial pressures of these four gases in a sample of air at
A 35.8 L cylinder of Ar(g) is connected to an evacuated 1875 L tank. If the temperature is held constant and the final pressure is 721 mmHg, what must have been the original gas pressure in the cylinder, in atmospheres?
(A) The reaction of aluminum with hydrochloric acid produces hydrogen gas. The balanced chemical equation for the reaction is given below.2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g)If 35.5 mL of H2(g) is collected over water at 26 °C and a barometric pressure of 755 mmHg, how many moles of HCl
Which is the greater speed, that of a bullet fired from a high-powered M-16 rifle (2180 mi/h) or the root-mean-square speed of H2 molecules at 25 °C?
A sample of N2(g) occupies a volume of 42.0 mL under the existing barometric pressure. Increasing the pressure by 85 mmHg reduces the volume to 37.7 mL. What is the prevailing barometric pressure, in millimeters of mercury?
(A) Which has the greater root-mean-square speed at 25 °C, NH3(g) or HCl(g)? Calculate urms for the one with the greater speed.(B) At what temperature are urms of H2 and the speed of the M-16 rifle bullet given in Example 6-14 the same?Example 6-14Which is the greater speed, that of a bullet fired
If 2.2 x 10-4 mol N2(g) effuses through a tiny hole in 105 s, then how much H2(g) would effuse through the same orifice in 105 s?
A weather balloon filled with He gas has a volume of 2.00 x 103 m3 at ground level, where the atmospheric pressure is 1.000 atm and the temperature 27 °C. After the balloon rises high above Earth to a point where the atmospheric pressure is 0.340 atm, its volume increases to 5.00 x 103 m3. What is
(A) In Example 6-15, how much O2(g) would effuse through the same orifice in 105 s?(B) In Example 6-15, how long would it take for 2.2 x 10-4 mol H2 to effuse through the same orifice as the 2.2 x 10-4 mol N2?Example 6-15If 2.2 x 10-4 mol N2(g) effuses through a tiny hole in 105 s, then how much
A sample of Kr(g) escapes through a tiny hole in 87.3 s. The same amount of an unknown gas escapes in 42.9 s under identical conditions. What is the molar mass of the unknown gas?
The photographs show the contraction of an argon-filled balloon when it is cooled by liquid nitrogen. To what approximate fraction of its original volume will the balloon shrink when it is cooled from a room temperature of 22 °C to a final temperature of about -22 °C?
(A) Under the same conditions as in Example 6-16, another unknown gas requires 131.3 s to escape. What is the molar mass of this unknown gas?(B) Given all the same conditions as in Example 6-16, how long would it take for a sample of ethane gas, C2H6, to effuse?Example 6-16A sample of Kr(g) escapes
Use the van der Waals equation to calculate the pressure exerted by 1.00 mol Cl2(g) confined to a volume of 2.00 L at 273 K. For Cl2, a = 6.34 bar L2 mol-2 and b = 0.0542 L mol-1.
What is the mass of argon gas in a 75.0 mL volume at STP?
(A) Substitute CO2(g) for Cl2(g) in Example 6-17, given the values a = 3.66 bar L2 mol-2 and b = 0.0429 L mol-1. Which gas, CO2 or Cl2, shows the greater departure from ideal gas behavior?(B) Substitute CO(g) for Cl2(g) in Example 6-17, given the values a = 1.47 bar L2 mol-2 and b = 0.0395 L mol-1.
What volume of gaseous chlorine at STP would you need to obtain a 250.0 g sample of gas?
(A) When a 0.5120 g sample of a gaseous hydrocarbon was burned in excess oxygen, 1.687 g CO2 and 0.4605 g H2O were obtained. The density of the compound, in its vapor form, is 1.637 g/L at 25 °C and 101.3 kPa. Determine the molecular formula of the hydrocarbon, and draw a plausible structural
A 27.6 mL sample of PH3(g) (used in the manufacture of flame-retardant chemicals) is obtained at STP.(a) What is the mass of this sample, in milligrams?(b) How many molecules of PH3 are present?
A 5.0 x 1017 atom sample of radon gas is obtained.(a) What is the mass of this sample, in micrograms?(b) What is the volume of this sample at STP, in microliters?
The Haber process is the principal method for fixing nitrogen (converting N2 to nitrogen compounds).Assume that the reactant gases are completely converted to NH3(g) and that the gases behave ideally.(a) What volume of NH3(g) can be produced from 152 L N2(g) and 313 L of H2(g) if the gases are
You purchase a bag of potato chips at an ocean beach to take on a picnic in the mountains. At the picnic, you notice that the bag has become inflated, almost to the point of bursting. Use your knowledge of gas behavior to explain this phenomenon.
What is the volume, in liters, occupied by a mixture of 15.2 g Ne(g) and 34.8 g Ar(g) at 7.24 bar pressure and 26.7 °C?
A balloon filled with H2(g) at and 1.00 atm has a volume of 2.24 L. What is the final gas volume if 0.10 mol He(g) is added to the balloon and the temperature is then raised to 100 °C while the pressure and amount of gas are held constant?
A gas cylinder of 53.7 L volume contains N2(g) at a pressure of 28.2 atm and 26 °C. How many grams of Ne(g) must we add to this same cylinder to raise the total pressure to 75.0 atm?
In the drawing it shown that, 1.00 g H2(g) at 300 K 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 0.50 g H2(g) is added and the temperature is reduced to 275 K? Explain your answer. 1.00
A 2.35 L container of H2(g) at 762 mmHg and 24 °C is connected to a 3.17 L container of He(g) at 728 mmHg and 24 °C. After mixing, what is the total gas pressure, in millimeters of mercury, with the temperature remaining at 24 °C?
Consider the statements (a) to (e) below. Assume that H2(g) and O2(g) behave ideally. State whether each of the following statements is true or false. For each false statement, explain how you would change it to make it a true statement.(a) Under the same conditions of temperature and pressure, H2
Draw a box to represent a sample of air containing N2 molecules (represented as squares) and O2 molecules (represented as circles) in their correct proportions. How many squares and circles would you need to draw to also represent the CO2(g) in air through a single mark? What else should you add to
The concentration of Mn2+(aq) can be determined by titration with MnO4-(aq) in basic solution. A 50.00 mL sample of Mn2+(aq) requires 78.42 mL of 0.04997 M KMnO4 for its titration. What is [Mn2+] in the sample?Mn2+ + MnO4- → MnO2(s) (not balanced)
The titration of 5.00 mL of a saturated solution of sodium oxalate, Na2C2O4, at 25 °C requires 25.8 mL of 0.02140 M KMnO4 in acidic solution. What mass of Na2C2O4 in grams would be present in 1.00 L of this saturated solution?C2O42- + MnO4- → Mn2+ + CO2(g) (not balanced)
In the treatment of 1.00 x 102 L of a wastewater solution that is 0.0126 M CrO42- how many grams of (a) Cr(OH)3(s) would precipitate;(b) Na2S2O4 would be consumed?
Write net ionic equations for the reactions depicted in photo (a) Sodium metal reacts with water to produce hydrogen; photo (b) An excess of aqueous iron(III) chloride is added to the solution in (a); and photo (c) the precipitate from (b) is collected and treated with an excess of HCl(aq).
Scuba divers know that they must not ascend quickly from deep underwater because of a condition known as the bends. Another concern is that they must constantly exhale during their ascent to prevent damage to the lungs and blood vessels. Describe what would happen to the lungs of a diver who
A sample of gas has a volume of 4.25 L at 25.6 °C and 748 mmHg. What will be the volume of this gas at 26.8 °C and 742 mmHg?
A constant-volume vessel contains 12.5 g of a gas at 21 °C. If the pressure of the gas is to remain constant as the temperature is raised to 210 °C, how many grams of gas must be released?
A 10.0 g sample of a gas has a volume of 5.25 L at 25 °C and 102 kPa. If 2.5 g of the same gas is added to this constant 5.25 L volume and the temperature raised to 62 °C, what is the new gas pressure?
A 34.0 L cylinder contains 305 g O2(g) at 22 °C. How many grams of O2(g) must be released to reduce the pressure in the cylinder to 1.15 atm if the temperature remains constant?
What is the volume, in liters, occupied by 89.2 g CO2(g) at 37 °C and 98.3 kPa?
A 12.8 L cylinder contains 35.8 g O2 at 46 °C. What is the pressure of this gas, in kilopascals?
Kr(g) in a 18.5 L cylinder exerts a pressure of 11.2 atm at 28.2 °C. How many grams of gas are present?
A 72.8 L constant-volume cylinder containing 7.41 g He is heated until the pressure reaches 3.50 atm. What is the final temperature in degrees Celsius?
A laboratory high vacuum system is capable of evacuating a vessel to the point that the amount of gas remaining is 5.0 x 109 molecules per cubic meter. What is the residual pressure in pascals?
What is the pressure, in pascals, exerted by 1242 g CO2(g) when confined at -25 °C to a cylindrical tank 25.0 cm in diameter and 1.75 m high?
At what temperature is the molar volume of an ideal gas equal to 22.4 L, if the pressure of the gas is 2.5 atm?
What is the molar volume of an ideal gas at (a) 25 °C and 1.00 atm; (b) 100 °C and 748 Torr?
A 0.418 g sample of gas has a volume of 115 mL at 66.3 °C and 99.0 kPa. What is the molar mass of this gas?
What is the molecular formula of a gaseous fluoride of sulfur containing 70.4% F and having a density of approximately 4.5 g/L at 20 °C and 1.0 atm?
What is the molar mass of a gas found to have a density of 0.841 g/L at 415 K and 96.7 kPa?
A gaseous hydrocarbon weighing 0.231 g occupies a volume of 102 mL at 23 °C and 749 mmHg. What is the molar mass of this compound? What conclusion can you draw about its molecular formula?
A 2.650 g sample of a gaseous compound occupies 428 mL at 24.3 °C and 742 mmHg. The compound consists of 15.5% C, 23.0% Cl, and 61.5% F, by mass. What is its molecular formula?
A 132.10 mL glass vessel weighs 56.1035 g when evacuated and 56.2445 g when filled with the gaseous hydrocarbon acetylene at 749.3 mmHg and 20.02 °C. What is the molar mass of acetylene? What conclusion can you draw about its molecular formula?
A particular application calls for N2(g) with a density of 1.80 g/L at 32 °C. What must be the pressure of the N2(g) in millimeters of mercury? What is the molar volume under these conditions?
Monochloroethylene gas is used to make polyvinylchloride (PVC). It has a density of 2.56 g/L at 22.8 °C and 101 kPa. What is the molar mass of Monochloroethylene? What is the molar volume under these conditions?
In order for a gas-filled balloon to rise in air, the density of the gas in the balloon must be less than that of air.(a) Consider air to have a molar mass of 28.96 g/mol; determine the density of air at 25 °C and 1.00 atm, in g/L.(b) Show by calculation that a balloon filled with carbon dioxide
Refer to Exercise 43, and determine the minimum temperature to which the balloon described in part (b) would have to be heated before it could begin to rise in air.Exercise 43In order for a gas-filled balloon to rise in air, the density of the gas in the balloon must be less than that of air.(a)
The density of phosphorus vapor is 2.64 g/L at 310 °C and 1.03 bar. What is the molecular formula of the phosphorus under these conditions?
A particular gaseous hydrocarbon that is 82.7% C and 17.3% H by mass has a density of 2.33 g/L at 23 °C and 746 mmHg. What is the molecular formula of this hydrocarbon?
How many liters of H2(g) at STP are produced per gram of Al(s) consumed in the following reaction? 2 Al(s) + 6HCl(aq) → 2 AlCl3(aq) + 3H₂(g)
One method of removing CO2(g) from a spacecraft is to allow the CO2 to react with LiOH. How many liters of CO2(g) at 25.9 °C and 1.00 bar can be removed per kilogram of LiOH consumed? 2 LiOH(s) + CO2(g) Li₂CO3(s) + H₂O(1)
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 kg of this coal?
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