1 / 14

Ppt 17b, Continuation of Gases & Gas Laws

Ppt 17b, Continuation of Gases & Gas Laws . Individual Gas Laws Combine to Form the Ideal Gas Law . Ideal Gas Law Problems-I Find one variable if the other three are known (“one state” problem) Problems in which the state of a gas changes (“two state” problem).

mdyer
Télécharger la présentation

Ppt 17b, Continuation of Gases & Gas Laws

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Ppt 17b, Continuation of Gases & Gas Laws • Individual Gas Laws Combine to Form the Ideal Gas Law. • Ideal Gas Law Problems-I • Find one variable if the other three are known (“one state” problem) • Problems in which the state of a gas changes (“two state” problem). • Density of Gases Ideas & Calculations • Can use Ideal Gas Law here (or memorize variant) Ppt17b

  2. Important Comment • In all previous laws, the proportionality constant, k , is not a fundamental constant of nature; it would depend on the conditions [the values of the other variables being held constant] Ppt17b

  3. The Ideal Gas Law • Ideal gases obey an equation incorporating the laws of Charles, Boyle, and Avogadro: • The gas constant R = 0.08206 L·atm·K–1·mol–1 • STP conditions are 273.15 K and 1 atm pressure • 1 mole of an ideal gas occupies 22.41 Lat STP(molar volume = V of 1 mol) [same for all gases, conditions] Ppt17b

  4. The Ideal Gas Law No “before and after” kind of problem (1 state) • Sulfur hexafluoride (SF6) is a colorless, odorless, very unreactive gas. Calculate the pressure (in atm) exerted by 1.82 moles of the gas in a steel vessel of volume 5.43 L at 69.5°C. • What is the volume (in liters) occupied by 7.40 g of CO2 at STP? (Recall: STP is P = 1 atm; T = 0°C) Ppt17b

  5. What if a variable changes? (2 “states”!) A “before and after” kind of problem (2 states) • Oxygen gas is normally sold in 49.0 L steel containers at a pressure of 150.0 atm. What volume would the gas occupy if the pressure was reduced to 1.02 atm and the temperature raised from 20oC to 35oC? Ppt17b

  6. Example #2 • An inflated balloon with a volume of 0.55 L at sea level, where the pressure is 1.0 atm, is allowed to rise to a height of 6.5 km, where the pressure is about 0.40 atm. • 1) Assuming that the temperature remains constant, what is the final volume of the balloon? • 2) Assuming that the temperature at sea level is 22°C and the temperature at 6.5 km is -28°C, what is the final volume of the balloon? Ppt17b

  7. Gases Worksheet-I Practice • Proportional relationships / calculations Ppt17b

  8. The Ideal Gas Law—Applications Recall: At the same T and P, equal volumes of gases contain equal numbers of molecules. V n (P, T constant) • Implication? • The concentration of gas particles is “fixed” at a given T and P! = a fixed value (at a givenP & T, for any gas!) Ppt17b

  9. At the same T & P, [gas] is “fixed” (sample size does not matter)(identity of the gas does not matter) Same T & P  … He H2 He …same number of particles per L Ar Ppt17b

  10. Density of a gas at fixed T and P does depend on gas identity (molar mass)! • Density is “number density” x mass per particle • Which equals concentration x molar mass! This slide is intended to make a conceptual connection, not give you another equation to memorize! • One could substitute in for n/V here to get an equation that relates d, P, T, and MM, • but I don’t think it’s really “worth it” (see answer key comments)

  11. Summary (of prior few slides): At the same T&P, concentrationis constant, but density varies with MM Same # particles / L, but… He H2 He …different densities for different gaseous substances, because mass Ar Greatest density b/c greatest MM per particle (and thus per mole) varies!

  12. Practical Application: Will gases (or balloons filled with them) float or sink (in air)? MM is the key! • Air is about 80% N2 and 20% O2 MM(air)  29 g/mol Quiz: Would a neon balloon float or sink? Argon? Ppt17b

  13. The bottom line? Density of a gas depends on molar mass, T, & P, but not on “amount” Since amount does not matter, I prefer to PICK A CONVENIENT AMOUNT* to solve problems that relate to gas density and molar mass! No need to memorize or derive separate equations (although if you want to do so, more power to you!) * 1 L of gas, if density is given; 1 mol of gas, if molar mass (or formula) is given Ppt17b

  14. The Ideal Gas Law—Applications (Examples) What is the molar mass of a gas with a density of 4.07 g/L at a pressure of 3.42 atm and 35°C? What is the density of uranium hexafluoride, UF6, (MM = 352 g/mol) under conditions of STP? To what temperature must a sample of CO2 be raised at 1.97 atm in order for the density to become 3.38 g/L? Ppt17b

More Related