ll

15) The volume of 350. mL of gas at 25°C is decreased to 135 mL at constant pressure. What is the final temperature of the gas? A) -158°C B) 9.6°C C) 65°C D) 500°C

A) -158°C

18) A balloon filled with helium gas at 20°C occupies 4.91 L at 1.00 atm. The balloon is immersed in liquid nitrogen at -196°C, while the pressure is raised to 5.20 atm. What is the volume of the balloon in the liquid nitrogen? A) 0.25 L B) 3.6 L C) 6.7 L' D) 97 L

A) 0.25 L

11) A sample of 0.200 moles of nitrogen occupies 0.400 L. Under the same conditions, what number of moles occupies 1.200 L? A) 0.600 moles B) 0.0667 moles C) 2.40 moles D) 0.0960 moles

A) 0.600 moles

30) A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm. What is the partial pressure of Ne? A) 1.1 atm B) 0.80 atm C) 0.54 atm D) 0.40 atm E) 1.3 atm

A) 1.1 atm

17) A basketball is inflated to a pressure of 1.90 atm in a 24.0°C garage. What is the pressure of the basketball outside where the temperature is -1.00°C? A) 1.74 atm B) 1.80 atm C) 2.00 atm D) 2.08 atm

A) 1.74 atm

21) Determine the density of CO2 gas at STP. A) 1.96 g/L B) 1.80 g/L C) 2.24 g/L D) 4.46 g/L E) 5.10 g/L

A) 1.96 g/L

14) A sample of gas initially has a volume of 859 mL at 565 K and 2.20 atm. What pressure will the sample have if the volume changes to 268 mL while the temperature is increased to 815 K? A) 10.2 atm B) 9.83 atm C) 15.3 atm D) 6.53 atm E) 1.05 atm

A) 10.2 atm

39) Determine the mass of water formed when 12.5 L NH3 (at 298 K and 1.50 atm) is reacted with 18.9 L of O2 (at 323 K and 1.1 atm). 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) A) 17.0 g H2O B) 20.7 g H2O C) 37.7 g H2O D) 13.8 g H2O E) 27.9 g H2O

A) 17.0 g H2O

37) Determine the theoretical yield and the percent yield if 21.8 g of K2CO3 is produced from reacting 27.9 g KO2 with 29.0 L of CO2 (at STP). The molar mass of KO2 = 71.10 g/mol and K2CO3 = 138.21 g/mol. 4 KO2(s) + 2 CO2(g) → 2 K2CO3(s) + 3 O2(g) A) 27.1 g, 80.4 % yield B) 179 g, 12.2 % yield C) 91.7 g, 23.8 % yield D) 206 g, 10.6 % yield E) 61.0 g, 35.7 % yield

A) 27.1 g, 80.4 % yield

13) A gas is at 35.0°C and 3.50 L. What is the temperature at 7.00 L? A) 343°C B) 70.0°C C) 616°C D) 1.16°C E) 17.5°C

A) 343°C

15) What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C? A) 4.1 atm B) 5.0 atm C) 6.4 atm D) 1.1 atm E) 2.3 atm

A) 4.1 atm

12) To what volume will a sample of gas expand if it is heated from 50.0∘C and 2.33 L to 500.0°C? A) 5.58 L B) 23.3 L C) 0.233 L D) 0.97 L E) 0.184 L

A) 5.58 L

6) What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 742 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere? A) 656 mm Hg B) 733 mm Hg C) 751 mm Hg D) 828 mm Hg

A) 656 mm Hg

5) The atmospheric pressure is 715 mm Hg. What is the pressure in torr? A) 715 torr B) 28.1 torr C) 13.8 torr D) 31.8 torr E) 760 torr

A) 715 torr

14) A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle's law to calculate the pressure (torr) when the volume is reduced to 7.88 L at a constant temperature of 25.0°C. A) 846 torr B) 0.118 torr C) 5.26 × torr D) 526 torr E) 1.11 torr

A) 846 torr

5) The volume of a gas is proportional to number of moles of a gas is known as A) Avogadro's Law B) Ideal Gas Law C) Charles's Law D) Boyle's Law E) Dalton's Law

A) Avogadro's Law

41) A mixture of 1.0 mol He and 1.0 mol Ne are at STP in a rigid container. Which of the following statements is TRUE? A) Both gases have the same average kinetic energy. B) Both gases contribute equally to the density of the mixture under these conditions. C) Both gases have the same molecular speed. D) The mixture has a volume of 22.4 L E) All of the above are TRUE.

A) Both gases have the same average kinetic energy.

1) An instrument used to atmospheric pressure is called a A) barometer B) manometer C) sphygmomanometer D) spectrophotometer E) spectrometer

A) barometer

7) If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mm Hg, the level of mercury in the tube will A) be 118 mm higher in the arm open to the atmosphere. B) be 118 mm higher in the arm connected to the gas cylinder. 'C) be 870 mm higher in the arm open to the atmosphere. D) be 870 mm higher in the arm connected to the gas cylinder.

A) be 118 mm higher in the arm open to the atmosphere.

26) Define hypoxia. A) oxygen starvation B) increased oxygen concentration in body tissues C) increased nitrogen concentration in body tissues and fluids D) nitrogen starvation

A) oxygen starvation

22) Determine the density of NH3 gas at 435 K and 1.00 atm. A) 2.10 g/L B) 0.477 g/L C) 0.321 g/L D) 2.24 g/L E) 0.851 g/L

B) 0.477 g/L

4) The volume of a gas is proportional to the temperature of a gas is known as A) Avogadro's Law B) Ideal Gas Law C) Charles's Law D) Boyle's Law E) Dalton's Law

C) Charles's Law

23) A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.41 atm. What is the 5 identity of the halogen? A) Br2 B) F2 C) Cl2 D) I2 E) Ge

C) Cl2

42) Which statement is TRUE about kinetic molecular theory? A) A single particle does not move in a straight line. B) The size of the particle is large compared to the volume. C) The collisions of particles with one another is completely elastic. D) The average kinetic energy of a particle is not proportional to the temperature.

C) The collisions of particles with one another is completely elastic.

3) An instrument used to measure blood pressure is called a A) barometer B) manometer C) sphygmomanometer D) spectrophotometer E) spectrometer

C) sphygmomanometer

6) The volume of a gas is inversely proportional to the pressure of a gas is known as A) Avogadro's Law B) Ideal Gas Law C) Charles's Law D) Boyle's Law E) Dalton's Law

D) Boyle's Law

47) The rate of effusion of oxygen to an unknown gas is 0.935. What is the other gas? A) Ne B) Ar C) F2 D) N2

D) N2

7) A scuba diver experiences ________ as she descends into the ocean water. A) decrease of 1 atm for each 20 m of depth B) decrease of 1 atm for each 10 m of depth C) increase of 1 atm for each 20 m of depth D) increase of 1 atm for each 10 m of depth E) no difference in pressure

D) increase of 1 atm for each 10 m of depth

51) This equation is used to calculate the properties of a gas under nonideal conditions. A) Charles's Law B) Avogadro's Law C) Boyle's Law D) van der Waals equation E) Dalton's Law

D) van der Waals equation

16) A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr. A) 10.9 L B) 13.2 L C) 2.07 L D) 7.56 L E) 48.4 L

B) 13.2 L

29) A gas mixture consists of N2, O2, and Ne, where the mole fraction of N2 is 0.55 and the mole fraction of Ne is 0.25. If the mixture is at STP in a 5.0 L container, how many molecules of O2 are present? A) 4.5 ×1022 molecules O2 B) 2.7 ×1022 molecules O2 C) 3.7 × 1023 molecules O2 D) 1.1 ×1023 molecules O2 E) 9.3 × 1024 molecules O2

B) 2.7 ×1022 molecules O2

35) Determine the volume of H2S (at 375 K and 1.20 atm) needed to produce 55.0 g of S. Assume that there is excess SO2 present. 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g) A) 44.0 L B) 29.3 L C) 22.7 L D) 34.1 L E) 66.0 L

B) 29.3 L

19) What pressure (in atm) will 0.44 moles of CO2 exert in a 2.6 L container at 25°C? A) 0.35 atm B) 4.1 atm C) 4.7 atm D) 8.6 atm E) 3.6 atm

B) 4.1 atm

44) Calculate the root mean square velocity of nitrogen molecules at 25°C. A) 729 m/s B) 515 m/s C) 149 m/s D) 297 m/s

B) 515 m/s

40) Determine the total volume of all gases (at STP) formed when 50.0 mL of TNT (C3H5(NO3)3, d = 1.60 g/mL, molar mass = 227.10 g/mol) reacts according to the following reaction. 4 C3H5(NO3)3(l) → 6 N2(g) + O2(g) + 12 CO2(g) + 10 H2O(g) A) 4.93 L B) 57.2 L C) 29.6 L D) 448 L E) 175 L

B) 57.2 L

9) If a sample of 0.29 moles of Ar occupies 3.8 L under certain conditions, what volume will 0.66 moles occupy under the same conditions? A) 12 L B) 8.6 L C) 17 L D) 5.0 L E) 15 LB

B) 8.6 L

45) The rate of effusion of two different gases is known as A) Avogadro's Law B) Graham's Law C) Charles's Law D) Boyle's Law E) Dalton's Law

B) Graham's Law

50) Which of the following compounds will behave LEAST like an ideal gas at low temperatures? A) He B) SO2 C) H2 D) N2 E) F2

B) SO2

46) Give the definition for diffusion. A) gas molecules mix equally B) gas molecules spread out in a concentration gradient C) gas molecules escape from a container into a vacuum through a small hole D) average distance between collisions E) gas molecules mix unequally

B) gas molecules spread out in a concentration gradient

2) An instrument used to measure the pressure of a gas in a laboratory is called a A) barometer B) manometer C) sphygmomanometer D) spectrophotometer E) spectrometer

B) manometer

27) Define vapor pressure. A) partial pressure of water in a liquid mixture B) partial pressure of water in a gaseous mixture C) condensation of water D) water dissolved in a liquid E) water molecules

B) partial pressure of water in a gaseous mixture

31) The following reaction is used to generate hydrogen gas in the laboratory. If 243 mL of gas is collected at 25°C and has a total pressure of 745 mm Hg, what mass of hydrogen is produced? A possibly useful table of water vapor pressures is provided below. Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) A) 0.0196 g H2 B) 0.0717 g H2 C) 0.0190 g H2 D) 0.0144 g H2 E) 0.0449 g H2 Answer: CDiff: 3 Page Ref: 5.6 T (°C) 20 25 30 P (mm Hg) 17.55 23.78 31.86

C) 0.0190 g H2

10) A syringe contains 0.65 moles of He gas that occupy 750.0 mL. What volume (in L) of gas will the syringe hold if 0.35 moles of Ne is added? A) 0.87 L B) 4.9 L C) 1.2 L D) 2.1 L E) 1.9 L

C) 1.2 L

32) A syringe contains 589 mL of CO at 325 K and 1.2 atm pressure. A second syringe contains 473 7 mL of N2 at 298 K and 2.6 atm. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at STP? A) 0.59 atm B) 1.1 atm C) 1.7 atm D) 1.9 atmE) 3.8 atm

C) 1.7 atm

1) Convert 1.50 atm to mm Hg. A) 760 mm Hg B) 875 mm Hg C) 1140 mm Hg D) 1000 mm Hg E) 1520 mm Hg

C) 1140 mm Hg

2) Convert 1.50 atm to torr. A) 760 torr B) 875 torr C) 1140 torr D) 1000 torr E) 1520 torr

C) 1140 torr

10) A gas occupies 4.23 L at 2.25 atm. What is the volume at 3.46 atm? A) 6.50 L B) 1.84 L C) 2.75 L D) 32.9 L E) 0.364 L

C) 2.75 L

36) How many molecules of XeF6 are formed from 12.9 L of F2 (at 298 K and 2.60 atm) according to the following reaction? Assume that there is excess Xe. Xe(g) + 3 F2(g) → XeF6(g) A) 1.21 × 1023 molecules XeF6 B) 8.25 × 1023 molecules XeF6 C) 2.75 × 1023 molecules XeF6 D) 7.29 × 1023 molecules XeF6 E) 1.37 × 1023 molecules XeF6

C) 2.75 × 1023 molecules XeF6

3) Convert 1.75 atm to psi. A) 52.4 psi B) 875 psi C) 25.7 psi D) 1000 psi E) 1330 psi

C) 25.7 psi

9) What volume will a balloon occupy at 1.0 atm, if the balloon has a volume of 8.8 L at 4.4 atm? A) 2.0 L B) 0.50 L C) 39 L D) 13 LE) 4.4 L

C) 39 L

48) Which of the following statements is TRUE? A) Particles of different masses have the same average speed at a given temperature .B) The larger a molecule, the faster it will effuse. C) At very high pressures, a gas will occupy a larger volume than predicted by the ideal gas law. D) For a given gas, the lower the temperature, the faster it will effuse. E) None of the above statements are true.

C) At very high pressures, a gas will occupy a larger volume than predicted by the ideal gas law.

34) Determine the volume of O2 (at STP) formed when 50.0 g of KClO3 decomposes according to the following reaction. The molar mass for KClO3 is 122.55 g/mol. 2 KClO3(s) → 2 KCl(s) + 3 O2(g) A) 9.14 L B) 8.22 L C) 12.3 L D) 13.7 L E) 14.6 L

D) 13.7 L

4) The atmospheric pressure is 700 mm Hg. What is the pressure in inches of Hg? A) 16.0 in Hg B) 0.921 in Hg C) 13.5 in Hg D) 27.6 in Hg E) 32.5 in Hg

D) 27.6 in Hg

24) A 0.465 g sample of an unknown compound occupies 245 mL at 298 K and 1.22 atm. What is the molar mass of the unknown compound? A) 26.3 g/mol B) 33.9 g/mol C) 12.2 g/mol D) 38.0 g/mol E) 81.8 g/mol

D) 38.0 g/mol

12) A large balloon is initially filled to a volume of 25.0 L at 353 K and a pressure of 2575 mm Hg. What volume of gas will the balloon contain at 1.35 atm and 253 K? A) 22.2 L B) 87.5 L C) 11.4 L D) 45.0 L E) 58.6 L

D) 45.0 L

33) What pressure would a gas mixture in a 10.0 L tank exert if it were composed of 48.5 g He and 94.6 g CO2 at 398 K? A) 39.6 atm B) 7.02 atm C) 32.6 atm D) 46.6 atm E) 58.7 atm

D) 46.6 atm

8) A container filled with gas is connected to an open-end manometer that is filled with mineral oil. The pressure in the gas container is 753 mm Hg and atmospheric pressure is 724 mm. How high will the level rise in the manometer if the densities of Hg and mineral oil are 13.6 g/mL and 0.822 g/mL respectively? A) 1.75 mm B) 23.8 mm C) 29.0 mm D) 480 mm

D) 480 mm

8) What volume (in mL) will a sample of F2 gas occupy in a syringe at 5.5 atm, if the F2 has a volume of 25.0 mL at 1.2 atm? A) 11 mL B) 17 mL C) 3.8 mL D) 5.5 mL E) 7.6 mL

D) 5.5 mL

16) What mass of NO2 is contained in a 13.0 L tank at 4.58 atm and 385 K? 3 A) 18.8 g B) 53.1 g C) 24.4 g D) 86.7 g E) 69.2 g

D) 86.7 g

49) Which of the following statements is TRUE? A) At a given temperature, lighter gas particles travel more slowly than heavier gas particles. B) The smaller a gas particle, the slower it will effuse C) The higher the temperature, the lower the average kinetic energy of the sample. D) At low temperatures, intermolecular forces become important and the pressure of a gas will be lower than predicted by the ideal gas law. E) None of the above statements are true.

D) At low temperatures, intermolecular forces become important and the pressure of a gas will be lower than predicted by the ideal gas law.

17) What is the volume of 5.60 g of O2 at 7.78 atm and 415K? A) 1.53 L B) 565 L C) 24.5 L D) 25.0 L E) 0.766 L

E) 0.766 L

38) Determine the volume of SO2 (at STP) formed from the reaction of 96.7 g of FeS2 and 55.0 L of O2 (at 398 K and 1.20 atm). The molar mass of FeS2 is 119.99 g/mol. 4 FeS2(s) + 11 O2(g) → 2 Fe2O3(s) + 8 SO2(g) A) 36.1 L B) 45.3 L C) 18.1 L D) 27.6 L E) 32.9 L

E) 32.9 L

13) A syringe initially holds a sample of gas with a volume of 285 mL at 355 K and 1.88 atm. To what temperature must the gas in the syringe be heated/cooled in order to have a volume of 435 mL at 2.50 atm? A) 139 K B) 572 K C) 175 K D) 466 K E) 721 K

E) 721 K

11) To what temperature must a balloon, initially at 25°C and 2.00 L, be heated in order to have a volume of 6.00 L? A) 993 K B) 403 K C) 75 K D) 655 K E) 894 K

E) 894 K

28) The total pressure of a gas mixture is the sum of the partial pressure of its components is known as A) Avogadro's Law B) Ideal Gas Law C) Charles's Law D) Boyle's Law E) Dalton's Law

E) Dalton's Law

20) Which of the following will cause the volume of an ideal gas to triple in value? A) Raising the temperature from 25°C to 75°C at constant pressure. B) Lowering the absolute temperature by a factor of 3 at constant pressure. C) Raising the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3. D) Lowering the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3. E) Lowering the pressure by a factor of 3 while the temperature stays constant.

E) Lowering the pressure by a factor of 3 while the temperature stays constant.

25) A compound is found to be 30.45% N and 69.55 % O by mass. If 1.63 g of this compound occupy 389 mL at 0.00°C and 775 mm Hg, what is the molecular formula of the compound? A) NO2 B) N2O C) N4O2 D) N2O5 E) N2O4

E) N2O4