Chapter 5b as handout

# Chapter 5b as handout - Density(d Calculations d is the...

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1 Density ( d ) Calculations d = m V m is the mass of the gas in g M is the molar mass in g/mol Molar Mass ( M ) of a Gaseous Substance dRT P = d is the density of the gas in g/L 5.4 d = m V = P RT m n = Example : A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm and 27.0 º C. What is the molar mass of the gas? 5.4 dRT P = d = m V = = Gas Stoichiometry Example : What is the volume of CO 2 produced at 37 0 C and 1.00 atm when 5.60 g of glucose are used up in the reaction: C 6 H 12 O 6 ( s ) + 6O 2 ( g ) 6CO 2 ( g ) + 6H 2 O ( l ) g C 6 H 12 O 6 mol C 6 H 12 O 6 mol CO 2 V CO 2 5.60 g C 6 H 12 O 6 1 mol C 6 H 12 O 6 180 g C 6 H 12 O 6 x 6 mol CO 2 1 mol C 6 H 12 O 6 x = 0.187 mol CO 2 V = nRT P = 5.5

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2 Dalton’s Law of Partial Pressures V and T are constant P 1 P 2 P total = P 1 + P 2 5.6 Consider a case in which two gases, A and B , are in a container of volume V. P A = n A RT V P B = n B RT V n A is the number of moles of A n B is the number of moles of B P T = P A + P B
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## This note was uploaded on 02/20/2012 for the course CHEM 1230 taught by Professor Anderson during the Spring '08 term at Toledo.

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Chapter 5b as handout - Density(d Calculations d is the...

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