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Transcript

The Ideal Gas Law:

g

PV

=

molar mass

RT

Calculating Percent Error

Experimental Value - Actual Value

x 100

% error =

PV

Actual Value

(62.3637) x (293.15)

R = 62.3637

T = 20°c = 293.15°K

Formula of Butane = C H

4 10

molar

mass

0.5198

x

=

PV = nRT

by adding 273.15 to convert into Kelvin

C = 12.011

H = 1.008

(728.5) x (0.22)

Actual Value =

4 x (12.011) + 10 x (1.008)

=

Finding the Partial Pressure of Dry Butane:

g/mol

58.124

P = P - P

250mL = the amount of water we started with

butane room water vapor

RT

30mL = the amount of water remaining in the bottle

The temperature of water was 20°c, so the water vapor pressure is 17.5 (in torrs)

250mL - 30mL = 220mL

The pressure of the room as measured on the barometer was 746 torrs

V =

P=

220mL = the volume of butane gas collected

P = 746 - 17.5

butane

Finding the Molar Mass of Butane

n =

0.22L

molar mass

=

59.29 g

P = 728.5

of butane gas collected

g

butane

59.29 - 58.124

molar

mass

x

=

x 100

% error =

Initial mass of lighter = 14.8805

Mass of lighter after = 14.3607

58.124

Mass of butane gas used = 14.8805 - 14.3607

G =

Mass of butane = 0.5198

PV

% error = 2.01%

RT

molar mass

n = Moles

=

R = The Universal Gas Constant

Which we can change to:

T = Temperature

P = Pressure

V = Volume

g

Grams

Since we are using torr for pressure, the universal gas constant we will use is

Which is always in Kelvin

We will use pressure in torr

Which is always in Liters

PV

Formula Mass

62.3637

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