Download presentation

Presentation is loading. Please wait.

Published byRachel Johnston Modified over 3 years ago

1
Ideal Gas Law The equality for the four variables involved in Boyle’s Law, Charles’ Law, Gay-Lussac’s Law and Avogadro’s law can be written PV = nRT R = ideal gas constant

2
Ideal Gases Behave as described by the ideal gas equation; no real gas is actually ideal Within a few %, ideal gas equation describes most real gases at room temperature and pressures of 1 atm or less In real gases, particles attract each other reducing the pressure Real gases behave more like ideal gases as pressure approaches zero.

3
**PV = nRT R is known as the universal gas constant Using STP conditions**

R = PV = (1.00 atm)(22.4 L) nT (1mol) (273K) n T = L-atm mol-K

4
Learning Check G15 What is the value of R when the STP value for P is 760 mmHg of 1 mole of gas?

5
Solution G15 What is the value of R when the STP value for P is 760 mmHg? R = PV = (760 mm Hg) (22.4 L) nT (1mol) (273K) = L-mm Hg mol-K

6
Learning Check G16 Dinitrogen monoxide (N2O), laughing gas, is used by dentists as an anesthetic. If 2.86 mol of gas occupies a 20.0 L tank at 23°C, what is the pressure (mmHg) in the tank in the dentist office?

7
**Solution G16 Adjust to match the units of R**

Set up data for 3 of the 4 gas variables Adjust to match the units of R V = L L T = 23°C K n = mol 2.86 mol P = ? ?

8
**Rearrange ideal gas law for unknown P**

P = nRT V Substitute values of n, R, T and V and solve for P P = (2.86 mol)(62.4L-mmHg)(296 K) (20.0 L) (K-mol) = x 103 mm Hg

9
Learning Check G17 A 5.0 L cylinder contains oxygen gas at 20.0°C and 735 mm Hg. How many grams of oxygen are in the cylinder?

10
**Solution G17 Solve ideal gas equation for n (moles) n = PV RT**

= (735 mmHg)(5.0 L)(mol K) (62.4 mmHg L)(293 K) = mol O2 x g O2 = 6.4 g O2 1 mol O2

11
**Molar Mass of a gas n = PV = (0.813 atm) (0.215 L) = 0.00703 mol**

What is the molar mass of a gas if g of the gas occupy 215 mL at atm and 30.0°C? n = PV = (0.813 atm) (0.215 L) = mol RT ( L-atm/molK) (303K) Molar mass = g = g = g/mol mol mol

12
Density of a Gas Calculate the density in g/L of O2 gas at STP. From STP, we know the P and T. P = atm T = 273 K Rearrange the ideal gas equation for moles/L PV = nRT PV = nRT P = n RTV RTV RT V

13
Substitute (1.00 atm ) mol-K = mol O2/L ( L-atm) (273 K) Change moles/L to g/L mol O2 x g O2 = g/L 1 L mol O2 Therefore the density of O2 gas at STP is 1.43 grams per liter

14
Formulas of Gases A gas has a % composition by mass of 85.7% carbon and 14.3% hydrogen. At STP the density of the gas is 2.50 g/L. What is the molecular formula of the gas?

15
**Formulas of Gases Calculate Empirical formula**

85.7 g C x 1 mol C = mol C/7.14 = 1 C 12.0 g C 14.3 g H x 1 mol H = 14.3 mol H/ 7.14 = 2 H 1.0 g H Empirical formula = CH2 EF mass = (1.0) = 14.0 g/EF

16
**Using STP and density ( 1 L = 2.50 g)**

2.50 g x L = g/mol 1 L mol n = EF/ mol = g/mol = 4 14.0 g/EF molecular formula CH2 x = C4H8

17
**Gases in Chemical Equations**

On December 1, 1783, Charles used 1.00 x 103 lb of iron filings to make the first ascent in a balloon filled with hydrogen Fe(s) + H2SO4(aq) FeSO4(aq) + H2(g) At STP, how many liters of hydrogen gas were generated?

18
**Solution lb Fe g Fe mol Fe mol H2 L H2**

1.00 x 103 lb x g x 1 mol Fe x 1 mol H2 1 lb g mol Fe x L H2 = x 105 L H2 1 mol H2 Charles generated 182,000 L of hydrogen to fill his air balloon.

19
Learning Check G18 How many L of O2 are need to react 28.0 g NH3 at 24°C and atm? 4 NH3(g) + 5 O2(g) NO(g) H2O(g)

20
**Solution G18 Find mole of O2 28.0 g NH3 x 1 mol NH3 x 5 mol O2**

17.0 g NH mol NH3 = 2.06 mol O2 V = nRT = (2.06 mol)(0.0821)(297K) = L P atm

21
**Summary of Conversions with Gases**

Volume A Volume B Grams A Moles A Moles B Grams B Atoms or Atoms or molecules A molecules B

22
**Daltons’ Law of Partial Pressures**

The % of gases in air Partial pressure (STP) 78.08% N mmHg 20.95% O mmHg 0.94% Ar mmHg 0.03% CO mmHg PAIR = PN + PO + PAr + PCO = 760 mmHg Total Pressure mm Hg

23
Learning Check G19 A.If the atmospheric pressure today is 745 mm Hg, what is the partial pressure (mm Hg) of O2 in the air? 1) ) ) 760 B. At an atmospheric pressure of 714, what is the partial pressure (mm Hg) N2 in the air? 1) ) )

24
Solution G19 A.If the atmospheric pressure today is 745 mm Hg, what is the partial pressure (mm Hg) of O2 in the air? 2) 156 B. At an atmospheric pressure of 714, what is the partial pressure (mm Hg) N2 in the air? 1) 557

25
**Partial Pressure Partial Pressure**

Pressure each gas in a mixture would exert if it were the only gas in the container Dalton's Law of Partial Pressures The total pressure exerted by a gas mixture is the sum of the partial pressures of the gases in that mixture. PT = P P P

26
**Partial Pressures The total pressure of a gas mixture depends**

on the total number of gas particles, not on the types of particles. STP P = atm P = atm 0.50 mol O2 mol He mol N2 1.0 mol He

27
Health Note When a scuba diver is several hundred feet under water, the high pressures cause N2 from the tank air to dissolve in the blood. If the diver rises too fast, the dissolved N2 will form bubbles in the blood, a dangerous and painful condition called "the bends". Helium, which is inert, less dense, and does not dissolve in the blood, is mixed with O2 in scuba tanks used for deep descents.

28
Learning Check G20 A 5.00 L scuba tank contains 1.05 mole of O2 and mole He at 25°C. What is the partial pressure of each gas, and what is the total pressure in the tank?

29
**Solution G20 P = nRT PT = PO + PHe V 2**

PT = mol x L-atm x 298 K 5.00 L (K mol) = 7.19 atm

Similar presentations

OK

GAS LAWS. The Nature of Gases Gases expand to fill their containers Gases are fluid – they flow Gases have low density 1/1000 the density of the.

GAS LAWS. The Nature of Gases Gases expand to fill their containers Gases are fluid – they flow Gases have low density 1/1000 the density of the.

© 2017 SlidePlayer.com Inc.

All rights reserved.

Ads by Google

Ppt on power system stability using facts Ppt on media revolutions Ppt on bond length formula Ppt on limits and continuity in calculus Ppt on time division switching pdf Ppt on as 14 amalgamation of companies Ppt on pi in maths what is median Ppt on different types of quadrilaterals and their properties Ppt on animals for kindergarten Ppt on media research club