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MOLECULAR DESIGN INSTITUTE I NEW YORK UNIVERSITY 1
- Exam 1 will be handed back in recitation tomorrow 3/
- All regrade requests must be submitted by Wednesday 3/22 (in lecture to me or to your recitation instructor)
- All requests must be accompanied by a completed regrade request form (on Brightspace - >Content-> Exam 1) - Exams will be entirely regraded if a regrade request is submitted – it is possible that your score will decrease - A subset of exams have been scanned – any modification of exam answers will result in a 0 and reported to the dean
Lecture 12 announcements
MOLECULAR DESIGN INSTITUTE I NEW YORK UNIVERSITY 2
- Average 57 +/- 23
- A curve of +10 points will
be applied
credit points can be
earned by filling out the
Brightspace survey by
Tuesday 3/7 at 5pm
Exam 1 Results
MOLECULAR DESIGN INSTITUTE I NEW YORK UNIVERSITY 4
- Module 5 is due tomorrow 3/8 at 11:59pm
- Module 6 is due Friday 3/24 at 11:59pm
- There will be a quiz in recitation tomorrow (3/8) on Chapter 5
Lecture 12 announcements, continued
Chapter 5: The Gas Laws
• Properties of Gases
• Measuring pressure
• Ideal Gas Law & Boyle’s Law
• Kinetic-Molecular Theory
• Real Gases
SAMPLE PROBLEM: USING IDEAL GAS LAW
PROBLEM: An organic chemist isolates a colorless liquid from a petroleum
sample. She places the liquid in a preweighed flask and puts the
flask in boiling water, causing the liquid to vaporize and fill the
flask with gas. She obtains the following data:
Calculate the molar mass of the liquid.
Volume ( V ) of flask = 213 mL T = 100.00°C P = 754 torr
mass of flask + gas = 78.416 g mass of flask = 77.834 g
Poll Everywhere question
SAMPLE PROBLEM: CALCULATING PARTIAL PRESSURES
A mixture of gases contains 4.46 mol of neon (Ne), 0.74 mol of
argon (Ar), and 2.15 mol of xeon (Xe). Calculate the partial
pressure of argon if the total pressure is 2.00 atm at a certain
temperature.
PROBLEM:
IDEAL GAS LAW – OTHER RELATIONSHIPS Temperature : Root-Mean-Square Speed (RMS, uRMS) :
RELATIONSHIP BETWEEN MOLAR MASS & MOLECULAR SPEED 3RT MM uRMS = At constant T, heavier particles will be moving slowly on average.
VAN DER WAALS EQUATION ! = #$% & − #( − )
& !
Chapter 6: Thermochemistry
• 6.1 Forms of energy & their interconversion
• 6.2 Enthalpy: changes at constant pressure
• 6.3 Calorimetry: Measuring the heat of a chemical or
physical change
• 6.4 Stoichiometry of thermochemical equations
• 6.5 Hess’s Law: finding ∆H of any reaction
• 6.6 Standard enthalpies of reaction ∆"
TYPES OF ENERGY Thermal Energy : the kinetic energy associated with the random motion of atoms and molecules. Kinetic Energy : energy available due to the motion of an object. Potential Energy : energy available due to the position of an object. (in a force field, e.g., gravity, electric field, magnetic field…) Chemical Energy : the form of energy stored within the structural units of chemical substances.
SYSTEMS AND SURROUNDINGS System: the part of the universe that is of interest to us. Surroundings: the remainder of the universe. Open: Closed: Isolated: The System can be:
