Lecture 9 (10am) Chapter 5 (Gases) September 29 2009

Lecture 9 (10am) Chapter 5 (Gases) September 29 2009 -...

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Reminder: Exam on Wednesday September 30 th (Tomorrow!) 1.Bring a number 2 pencil to the exam. 2.No Graphing Calculators will be allowed – bring a scientific calculator. 3.Please go to the correct room to take your exam: 1110-01 DCC 318 1110-04 DCC 330 1100-09 Sage 3303 1100-11 DCC 308 Extra Time Students Walker 3221
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The Exam on Wednesday September 30 will cover material from Chapters 3 and 4 (and 17.1 – 17.5, 18.1 – 18.3, 19.2, and 21.1) This material is covered in lectures 1- 7. The material from Chapter 5 that we cover in class prior to the exam WILL NOT BE ON THE FIRST EXAM!
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Chapter 5 – Gases continued Lecture 9 September 29 2009
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Dalton’s Law of Partial Pressures Example: A mixture of noble gases is placed in a container at STP. The container contains 4.80g of He, 12.0g of Ar, and 32.5g of Kr. What is the partial pressure of each gas if P tot = 1 atm?
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The partial pressures of a gaseous mixture are given below. What is the mole fraction of neon? Partial Pressures hydrogen 125 mmHg carbon dioxide 320 mmHg methane 210 mmHg neon 150 mmHg (A)0.186 (B) 0.150 (C) 0.229 (D)0.250 (E) 0.810
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Vapor Pressure: Collecting a gas over water
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Example to try: A small piece of zinc reacts with dilute HCl to form H 2 gas which is collected over water at 16 o C. The total pressure is adjusted to barometric pressure (752 torr) (Remember that a torr is equal to a mmHg.) What is the partial pressure of H 2 ?
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Example to try: A small piece of zinc reacts with dilute HCl to form H 2 gas which is collected over water at 16 o C. The total pressure is adjusted to barometric pressure (752 torr)
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Lecture 9 (10am) Chapter 5 (Gases) September 29 2009 -...

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