Chapter 5b.student version

Chapter 5b.student version - Density (d ) Calculations d= m...

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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 =
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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 M = d = m V = =
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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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Dalton’s Law of Partial Pressures V and T are constant P 1 P 2 P total = P 1 + P 2 5.6
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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 X A
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Chapter 5b.student version - Density (d ) Calculations d= m...

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