The National Weather Service routinely

Chemistry 1B Chapter 10 Worksheet – DaleyName___________________________________1) The National Weather Service routinelysupplies atmospheric pressure data to helppilots set their altimeters. The units the NWSuses for atmospheric pressure are inches ofmercury. A barometric pressure of 30.51inches of mercury corresponds to __________kPa.A) 103.3B) 77.50C) 775D) 1.020E) 16.014) A balloon originally had a volume of 4.39 Lat 44 °C and a pressure of 729 torr. Theballoon must be cooled to __________°C toreduce its volume to 3.78 L (at constantpressure).A) 38B) 0C) 546D) 72.9E) 2735) If 3.21 mol of a gas occupies 56.2 L at 44 °Cand 793 torr, 5.29 mol of this gas occupies__________ L under these conditions.A) 30.9B) 14.7C) 478D) 92.6E) 61.72) A closed-end manometer was attached to avessel containing argon. The difference in themercury levels in the two arms of themanometer was 12.2 cm. Atmosphericpressure was 783 mmHg. The pressure of theargon in the container was __________mmHg.A) 882B) 661C) 122D) 795E) 7716) A gas originally at 27 °C and 1.00 atmpressure in a 3.9 L flask is cooled at constantpressure until the temperature is 11 °C. Thenew volume of the gas is __________ L.A) 0.27B) 0.24C) 3.9D) 4.1E) 3.73) A sample of gas (24.2 g) initially at 4.00 atmwas compressed from 8.00 L to 2.00 L atconstant temperature. After the compression,the gas pressure was __________ atm.A) 2.00B) 16.0C) 1.00D) 8.00E) 4.001Chemistry 1B Chapter 10 Worksheet – Daley7) A sample of H2 gas (12.28 g) occupies 100.0 Lat 400.0 K and 2.00 atm. A sample weighing9.49 g occupies __________ L at 353 K and2.00 atm.A) 54.7B) 77.3C) 147D) 68.2E) 10910) The reaction of 50 mL of N2 gas with 150 mLof H2 gas to form ammonia via the equation:N2 (g) + 3H2 (g) → 2NH3 (g)will produce __________ mL of ammonia ifpressure and temperature are kept constant.A) 50B) 150C) 200D) 250E) 1008) If 50.75 g of a gas occupies 10.0 L at STP, 129.3g of the gas will occupy __________ L at STP.A) 3.92B) 5.08C) 50.8D) 12.9E) 25.511) The density of ammonia gas in a 4.32 Lcontainer at 837 torr and 45.0 °C is__________ g/L.A) 0.194B) 0.432C) 0.717D) 3.86E) 4.22 × 10-29) A sample of a gas originally at 25 °C and 1.00atm pressure in a 2.5 L container is allowed toexpand until the pressure is 0.85 atm and thetemperature is 15 °C. The final volume of thegas is __________ L.A) 2.1B) 2.8C) 3.0D) 0.38E) 2.612) A sample of gas (1.9 mol) is in a flask at 21 °Cand 697 mmHg. The flask is opened andmore gas is added to the flask. The newpressure is 795 mmHg and the temperature isnow 26 °C. There are now __________ mol ofgas in the flask.A) 3.5B) 1.6C) 2.9D) 0.28E) 2.12Chemistry 1B Chapter 10 Worksheet – Daley13) The density of N2O at 1.53 atm and 45.2 °C is__________ g/L.A) 1.76B) 2.58C) 9.99D) 18.2E) 0.38816) What volume (mL) of sulfur dioxide can beproduced by the complete reaction of 3.82 gof calcium sulfite with excess HCl (aq), whenthe final SO2 pressure is 827 torr at 44.0 °C?A) 1.39 × 10-4B) 1.00 × 10-3C) 761D) 578E) 0.10614) The molecular weight of a gas is __________g/mol if 3.5 g of the gas occupies 2.1 L at STP.A) 2.7 × 10-217) Ammonium nitrite undergoes thermaldecomposition to produce only gases:B) 41C) 5.5 × 103NH4NO2 (s) → N2 (g) + 2H2O (g)D) 4.6 × 102E) 37What volume (L) of gas is produced by thedecomposition of 35.0 g of NH4NO2 (s) at525 ° C and 1.5 atm?A) 160B) 24C) 15D) 47E) 7215) The volume of hydrogen gas at 38.0 °C and763 torr that can be produced by the reactionof 4.33 g of zinc with excess sulfuric acid is__________ L.A) 2.71 × 10-4B) 0.592C) 3.69 × 104D) 2.84E) 1.6918) A sample of He gas (3.0 L) at 5.6 atm and 25°C was combined with 4.5 L of Ne gas at 3.6atm and 25 °C at constant temperature in a9.0 L flask. The total pressure in the flask was__________ atm. Assume the initial pressurein the flask was 0.00 atm.A) 1.0B) 3.7C) 9.2D) 24E) 2.63Chemistry 1B Chapter 10 Worksheet – Daley19) Since air is a mixture, it does not have a“molar mass.” However, for calculationpurposes, it is possible to speak of its“effective molar mass.” (An effective molarmass is a weighted average of the molarmasses of a mixture’s components.) If air atSTP has a density of 1.285 g/L, its effectivemolar mass is __________ g/mol.A) 26.9B) 31.4C) 28.8D) 34.4E) 30.022) Sodium hydride reacts with excess water toproduce aqueous sodium hydroxide andhydrogen gas:NaH (s) + H2O (l) → NaOH (aq) +H2 (g)A sample of NaH weighing __________ g willproduce 982 mL of gas at 28.0 °C and 765torr, when the hydrogen is collected overwater. The vapor pressure of water at thistemperature is 28 torr.A) 0.960B) 2.93C) 0.925D) 925E) 0.038820) In a gas mixture of He, Ne, and Ar with atotal pressure of 8.40 atm, the mole fractionof Ar is __________ if the partial pressures ofHe and Ne are 1.50 and 2.00 atm,respectively.A) 0.417B) 0.238C) 0.179D) 0.357E) 0.58323) CO (5.00 g) and CO2 (5.00 g) were placed in a750.0 mL container at 50.0 °C. The partialpressure of CO2 in the container was__________ atm.A) 1.60B) 4.01C) 6.31D) 10.3E) 0.29221) A gas mixture of Ne and Ar has a totalpressure of 4.00 atm and contains 16.0 mol ofgas. If the partial pressure of Ne is 2.75 atm,how many moles of Ar are in the mixture?A) 5.00B) 11.0C) 6.75D) 12.0E) 9.2524) The root-mean-square speed of CO at 113 °Cis __________ m/s.A) 58.3B) 586C) 31.5D) 317E) 9934Chemistry 1B Chapter 10 Worksheet – Daley25) Which of the following statements aboutgases is false?A) Distances between molecules of gas arevery large compared to bond distanceswithin molecules.B) Non-reacting gas mixtures arehomogeneous.C) Gases expand spontaneously to fill thecontainer they are placed in.D) Gases are highly compressible.E) All gases are colorless and odorless atroom temperature.28) Standard temperature and pressure (STP), inthe context of gases, refers to __________.A) 273 K and 1 pascalB) 298 K and 1 torrC) 273 K and 1 atmD) 273 K and 1 torrE) 298 K and 1 atm29) The molar volume of a gas at STP is__________ L.A) 14.7B) 0.08206C) 62.36D) 1.00E) 22.426) Molecular compounds of low molecularweight tend to be gases at room temperature.Which of the following is most likely not agas at room temperature?A) LiClB) CH4C) H2D) HClE) Cl230) “Isothermal” means __________.A) at constant pressureB) at ideal temperature and pressureconditionsC) at constant temperatureD) that ΔHrxn = 0E) at variable temperature and pressureconditions27) Gaseous mixtures __________.A) are all heterogeneousB) can only contain isolated atomsC) are all homogeneousD) can only contain moleculesE) must contain both isolated atoms andmolecules5Chemistry 1B Chapter 10 Worksheet – Daley31) The pressure exerted by a column of liquid isequal to the product of the height of thecolumn times the gravitational constant timesthe density of the liquid, P = ghd. How higha column of water (d = 1.0 g/mL) would besupported by a pressure that supports a 713mm column of mercury (d = 13.6 g/mL)?A) 9.7 × 103 mm33) The kinetic-molecular theory predicts thatpressure rises as the temperature of a gasincreases because __________.A) the gas molecules collide morefrequently with the wallB) the gas molecules collide lessfrequently with the wallC) the gas molecules collide moreenergetically with the wallD) the average kinetic energy of the gasmolecules decreasesE) both the gas molecules collide morefrequently with the wall and the gasmolecules collide more energeticallywith the wallB) 14 mmC) 713 mmD) 1.2 × 104 mmE) 52 mm32) Which statement about atmospheric pressureis false?A) Atmospheric pressure prevents waterin lakes, rivers, and oceans fromboiling away.B) With an increase in altitude,atmospheric pressure increases as well.C) The warmer the air, the lower theatmospheric pressure.D) Air actually has weight.E) As air becomes thinner, its densitydecreases.34) A 255 mL round-bottom flask is weighed andfound to have a mass of 114.85 g. A fewmilliliters of an easily vaporized liquid areadded to the flask and the flask is immersedin a boiling water bath. All of the liquidvaporizes at the boiling temperature ofwater, filling the flask with vapor. When allof the liquid has vaporized, the flask isremoved from the bath, cooled, dried, andreweighed. The new mass of the flask andthe condensed vapor is 115.23 g. Which ofthe following compounds could the liquidbe? (Assume the ambient pressure is 1 atm.)A) C2H6B) C3H7OHC) C4H9OHD) C2H5OHE) C4H106Chemistry 1B Chapter 10 Worksheet – Daley35) The average kinetic energy of the particles ofa gas is directly proportional to __________.A) the particle massB) the square of the rms speedC) the square of the particle massD) the rms speedE) the square root of the rms speed38) Which one of the following gases would havethe highest average molecular speed at 25°C?A) O2B) SF 6C) CO2D) CH4E) N236) According to kinetic-molecular theory, inwhich of the following gases will theroot-mean-square speed of the molecules bethe highest at 200 °C?A) H2OB) SF 6C) HClD) Cl2E) None. The molecules of all gases havethe same root-mean-square speed atany given temperature.39) A 1.44-g sample of an unknown pure gasoccupies a volume of 0.335 L at a pressure of1.00 atm and a temperature of 100.0 °C. Theunknown gas is __________.A) argonB) heliumC) kryptonD) xenonE) neon40) Given the equationC2H6 (g) + O2 (g) → CO 2 (g) + H2O (g)Determine the number of liters of O237) According to kinetic-molecular theory, if thetemperature of a gas is raised from 100 °C to200 °C, the average kinetic energy of the gaswill __________.A) decrease by a factor of 100B) increase by a factor of 100C) increase by a factor of 1.27D) decrease by halfE) doubleconsumed at STP when 270.0 grams of C2H6is burned.7

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