Unit+10+-+Gas+Laws

Gas Laws

A. 0.217 atm B. 0.466 atm  C. 0.613 atm 760 torr = 1 atm D. 1.63 atm E. 4.60 atm A. Charles's  B. Boyle's (P1 x V1 = P2 x V2) Pressure x Volume = Constant C. Amontons's D. Avogadro's E. Gay-Lussac's  A. Charles's V1/T1 = V2/T2 Volume = Constant x Temperature B. Boyle's C. Amontons's D. Avogadro's E. Dalton's A. Charles's B. Graham's C. Boyle's D. Avogadro's  E. Dalton's Volume and temperature are constant A. 10 torr  B. 50 torr Because as volume increases pressure decreases and as volume decreases pressure increases proportionally. C. 100 torr D. 200 torr E. 1000 torr  A. 4.0 L Because as volume increases pressure decreases and as volume decreases pressure increases proportionally. B. 6.0 L C. 9 L D. 36 L E. 48 L A. 22.3 L  B. 31.2 L Use the ideal gas law PV= nRT Must find the moles first then plug in the moles and new value to solve C. 44.9 L D. 112 L E. 380 L A. 212 torr Use the ideal gas law PV= nRT Must find the moles first then plug in the moles and new value to solve B. 289 torr C. 356 torr D. 441 torr E. 359 torr A. 5.38 L B. 10.9 L C. 19.0 L  D. 38.3 L Use the ideal gas law PV = nRT E. 77.9 L A. 3.69 L  B. 11.6 L Use the ideal gas law PV= nRT Must find the moles first then plug in the moles and new value to solve C. 20.2 L D. 63.5 L E. not possible, since the volume would have to be negative A. 0 K and l atm  B. 273.15 K and 760 torr The conditions 0 C and 1 atm are at stp C. 0°C and 760 atm D. 273.15°C and 760 torr E. none of these choices is correct  A. 80.0 torr Use Dalton's Law and the formula Pa = naRT/ V B. 200. torr C. 256 torr D. 500. torr E. 556 torr A. 75 torr B. 100. torr C. 150. torr  D. 200. torr Use Dalton's Law and the formulas //Xa= na/ na+nb// and //Pa = (Xa)(Pt)// and //Pa = naRT/ V// E. none of these choices is correct Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)  A. 2.24 L of H2 B. 4.48 L of H2 C. 5.60 L of H2 D. 11.2 L of H2 E. 22.4 L of H2  A. nitrogen the lower the atomic mass the faster the element effuses B. oxygen C. hydrogen chloride D. ammonia  E. carbon monoxide <span style="color: rgb(244, 37, 37)"> A. methane, CH4 the lower the atomic mass the faster the element effuses B. hydrogen sulfide, H2S C. carbon dioxide, CO2 D. water, H2O E. neon, Ne <span style="color: rgb(248, 22, 22)"> A. CHCl3 B. CH2Cl2 C. C2H2Cl2 D. C2H3Cl E. CCl4 A. O2 B. CO2 C. H2O D. H2 <span style="color: rgb(243, 22, 22)"> E. All have the same average kinetic energy. Any 2 gases at the same temp will have the same kenetic energy A. NH3 B. CO <span style="color: rgb(248, 13, 13)"> C. H2 the lowest mass will have the largest rms D. SF6<span style="color: rgb(10, 0, 2)"> <span style="color: rgb(12, 8, 8)"><span style="color: rgb(248, 48, 48)"><span style="color: rgb(10, 0, 2)"> E. All the gases have the same root-mean-square molecular speed at 25°C
 * 1) Hydrogen gas exerts a pressure of 466 torr in a container. What is this pressure in atmospheres?**
 * 2) "The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of moles" is a statement of** __**Law.**__
 * 3) "The volume of an ideal gas is directly proportional to its absolute temperature at constant pressure and number of moles" is a statement of Law.**
 * 4) "The total pressure in a mixture of unreacting gases is equal to the sum of the partial pressures of the individual gases" is a statement of Law.**
 * 5) A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100 torr, what is the new pressure?**
 * 6) A sample of the inert gas krypton has its pressure tripled while its temperature remained constant. If the original volume is 12 L, what is the final volume?**
 * 7) A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature?**
 * 8) A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?**
 * 9) A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123°C and 1.35 atm. What would be its volume at 468°C and 1.35 atm?**
 * 10) A sample of ammonia gas at 65.5°C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is -15.8°C and its pressure is 524 torr?**
 * 11) What are the conditions of STP?**
 * 12) A gas mixture consists of equal masses of methane (molecular weight 16.0) and argon (atomic weight 40.0). If the partial pressure of argon is 200. torr, what is the pressure of methane, in torr?**
 * 13) A gas mixture, with a total pressure of 300. torr, consists of equal masses of Ne (atomic weight 20.) and Ar (atomic weight 40.). What is the partial pressure of Ar, in torr?**
 * 14) Magnesium metal (0.100 mol) and a volume of aqueous hydrochloric acid that contains 0.500 mol of HCl are combined and react to completion. How many liters of hydrogen gas, measured at STP, are produced?**
 * 15) Which of the following gases effuses most rapidly?**
 * 16) Which of the following gases will be the slowest to diffuse through a room?**
 * 17) A compound composed of carbon, hydrogen, and chlorine effuses through a pinhole 0.411 times as fast as neon. Select the correct molecular formula for the compound.**
 * 18) Select the gas with the highest average kinetic energy per mole at 298 K.**
 * 19) Select the gas with the largest root-mean-square molecular speed at 25°C.**