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Chemistry Notes for Week 3

by: Bailey Wilhoit

Chemistry Notes for Week 3 Chem 111

Bailey Wilhoit


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These notes cover the parts of chapter 6 that were covered in class.
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This 3 page Class Notes was uploaded by Bailey Wilhoit on Sunday October 2, 2016. The Class Notes belongs to Chem 111 at University of South Carolina - Columbia taught by Stefik in Fall 2016. Since its upload, it has received 10 views. For similar materials see Chemsitry in Chemistry at University of South Carolina - Columbia.


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Date Created: 10/02/16
Chemistry Notes   Week 3    Chapter 6  6.1 Vocabulary  ● Pressure: force per unit area exerted on a surface  Important to Know:  ● Density of a solid is given in g/cm​  of g/mL  ● Density of a liquid is given in g/mL  ● Density of a gas is given in g/L  ● One atmosphere (atm) is the normal (standard) pressure at sea level. The SI unit  of pressure is the pascal (Pa)  2​ ○ 1 Pa = 1 kg ∕m(s​ ) (chemists hardly use pascals)  ○ 1 atm= 760 torr  ○ 1 atm= 14.7 psi  ○ 1 torr is equivalent to mmHg  6.2 Important to Know:  ● Boyle’s Law: as pressure increases, volume decreases  ○ P​1​ 1​ P​2​ 2  ● Charles’s Law: as volume increases, temperature increases  ○ P​1​T1​= P2​/T2  ● Gay Lussac’s Law: as pressure increases, temperature increases  ○ P​1​T1​= P2​/T2  ● Avogadro’s Hypothesis: equal volumes of gases at the same pressure and temperature  contain the same number of particles  ○ Pressures in both containers are the same, but the masses of the gases are  different  ● Combined Gas Law:  ○ P​1​ 1​T1​= P2​ 2​T​2  ○ Example: A gas occupies 5.00 L at 0.974 atm. Calculate the volume of gas at  1.00 atm when the temperature is constant.                                6.3 Important to Know:  ● Ideal Gas Law  ○ Pv=nRT  ○ P= pressure (in atm)  ○ v= volume  ○ n= moles  ○ R= 0.08206 (constant)  ○ T= temperature (K)  ● STP: T= 0°C, P= 1 atm  ● Ex:  ○ Calculate the molar mass of a gas if a 1.02 g sample at 220 mL at 95°C with a  pressure of 750 torr.                                    6.4 Important to Know:  ● The ideal gas law can be used to calculate the number of moles (n) in problems  ○ It relates n to the volume of gas as molar mass is used with masses of solids and  molarity is used with volumes of solutions  ● Ex:  ○ Calculate the volume of O​  g2​ formed in the decomposition of 2.21 g of KClO​   3 at STP      6.5 Vocabulary:  ● Partial pressure: pressure exerted by each gas in a mixture  ● Mole fraction (▯): number of moles of one component of a mixture divided by the  total number of moles of substances present in the mixture  Important to Know:  ● For a mixture of two gases (A and B) the total Pressure is:  ○ PT​= PA ​ P​B  ○ Ex: total pressure of a mixture of O and N is 4.51 atm. Experiment shows that O  is  present at 3.22 atm. Calculate the partial pressure of N  ■ 4.51 ­ 3.22 = 1.29   ● Mole fraction:  ○ ▯A​ + B​  +C​​  = 1 ( for a mix of 3 gases)  ○ The partial pressure of A in a mix is given by: P​A​= ▯A​ x PT    ● Ex: Calculate partial pressure of Ar gas in a container with 2.3 mol of Ar and 1.1 mol of  Ne with a total pressure of 1.4 atm.   


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