Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
Solve the equation

Transcribed Image Text:Here's the Third, and final, problem. You are doing an experiment in a laboratory that is 23°C
and 0.999 atm of pressure. You take a 0.995L flask that weighs 303.121g and fill it with CO2.
After it is filled it weighs 303.622g. Calculate the molar volume of the CO₂!
VSTP =
P₁V₁T STP
T₁P STP
0-999*0.995 * 273
296*1
= 0.916 L
1.200 * 0.995 = 1.1949
303.622-303-121 + 1.194 = 1.6959
1.695/44.01 = 0.0385 mol co₂
0.916/0.0385 = 23.79 L/mol
Mass of air = (density of air)(volume of flask)
1-200*0.995 = 1.1949
Mass of CO₂ = (Mass of flask filled with CO₂) - (Mass of empty flask) + (Mass of air)
303-622-303-121 +1-194 = 1.6959

Transcribed Image Text:Moles of CO₂ = (Mass of CO₂) ÷ (Molar Mass of CO₂)
1.695/44.01 = 0.0385
Molar Volume = VSTP + Moles of CO2
Percent error = |
0.916/0.0385 = 23-79 L/mol
experimental value-true value
true value
True value = 22.4 L/mol
x 100
22.4 23.79 * 100
22.4
6.205%
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