Chapter 9 - Part 2

# Chapter 9 - Part 2 - Chapter 9 Gases Lecture 20 (CHEM 1010)...

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Chapter 9 – Gases Lecture 20 (CHEM 1010) March 31 Agenda: Ideal Gas Law Applying the Ideal Gas Law Dalton’s Law of Partial Pressures Kinetic Molecular Theory of Gases Graham’s Law (Diffusion and Effusion Real world gas

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Pressure 1 atm = 760 mmHg = 1 torr = 101.325 kPa Boyle’s Law V inversely proportional to P Charles’ Law V directly proportional to T Avogadro’s Law V directly proportional to n Ideal Gas Law PV = nRT R can be 8.314 J/(K mol) or 8.314 kg m2/(s2 K mol) 0.08206 L atm/(K mol) Ideal Gas Law
Problem 9.68 challenge Pure oxygen gas was first prepared by heating mercury (II) oxide, HgO: 2HgO( s ) → 2Hg ( l ) + O2( g ) What volume (in liters) of oxygen at STP is released by heating 10.57 g of HgO?

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Problem 9.69 challenge How many grams of HgO would you need to heat if you wanted to prepare 0.0155 mol of O2 according to 2HgO( s ) → 2Hg ( l ) + O2( g ).
Propane gas (C3H8) is used as fuel in rural areas. How many liters of CO2 are formed at STP by the complete combustion of the propane in a container with a volume of 15.0L and a pressure of 4.5 atm at 25°C. The unbalance equation is C3H8(g) + O2(g)  CO2(g) + H2O(l) Gas Laws and Chemical Reactions Challenge 9.12 5th

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Propane gas (C3H8) is used as fuel in rural areas. How many liters of CO2 are formed at STP by the complete combustion of the propane in a container with a volume of 15.0L and a pressure of 4.5 atm at 25°C. The unbalance equation is C3H8(g) + O2(g)  CO2(g) + H2O(l) Gas Laws and Chemical Reactions Challenge 9.12 5th
Calculate the volume of oxygen in liters at 35°C and 630.0 mmHg, that could be obtained by heating 10.0 g of potassium chlorate (KClO3). Step #2 : # mols O2 = 0.1223 mol of O2 V = ?, R = 0.0821 L atm K-1 mol-1 T = 35 + 273 = 308 K, P = 630 / 760 = 0.82895 atm V = nRT/P V = [(0.1223mol)(0.0821L•atm•K-1•mol-1)(308K)]/0.82895atm = 3.73L Gas Laws and Chemical Reactions

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Dalton’s Law of Partial Pressures Many chemical problems involve mixtures of gases and not pure gases. In the case of gas mixtures the total gas pressure can be related to the pressures of individual gas components ( partial pressures ). Dalton’s Law of Partial pressures states:
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## Chapter 9 - Part 2 - Chapter 9 Gases Lecture 20 (CHEM 1010)...

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