Quantitative Properties of Gases. 1. Amount (mass or moles) 2. Volume 3. Pressure 4. Temperature
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1 Chapter 2 Gases
2 Quantitative Properties of Gases 1. Amount (mass or moles) 2. Volume 3. Pressure 4. Temperature
3 Kinetic Molecular Theory: (Video) Smallest particles (atoms, ions or molecules) of a substance are in continuous motion As particles move around they collide with each other and objects they touch Energy of motion is called kinetic energy Three types of motion: 1. Translational - straight line 2. Rotational - spinning or turning 3. Vibrational - back-and-forth, oscillating & bond flexion
4 Solid Definite shape & volume Virtually incompressible Does not flow Mainly vibrational motion Liquid Assumes container s shape Definite volume Virtually incompressible Flows readily Vibrational and rotational Gas Assumes container s shape and volume Highly compressible Flows readily Vibrational,rotational & translational motion
5 Particle Demonstration Tube: Predict what will happen when the mercury is heated strongly.
6 Diffusion : The process by which a substance spreads spontaneously in all directions from an area of high concentration to an area of lower concentration of the substance. Given this definition and the particle theory, predict what will happen when NO 2 gas is produced.
7 Experiment: Number of moles and the volume of a gas Purpose: The purpose of the experiment is to determine the relationship between the number of moles of H 2 gas produced in a reaction and the volume of H 2 gas. Hypothesis: The reaction is Mg (s) + 2HCl (aq) MgCl 2 (aq) + H 2(g) The independent variable is the. The dependent variable is the. The controlled variables are,, and. As the number of moles of H 2 gas produced increases, the volume of H 2 gas produced will. Procedure: Write a summary (pg. 12) don t copy word for word Diagram: Look at the apparatus label the diagram
8 Data: Volume-gas moles relationship Reaction Volume of HCl consumed (ml) ( ) Volume of water (ml) ( ) Moles of H 2 (g) produced (n) Volume of H 2 gas produced (ml) ( ) Volume of H 2 gas (ml) Class Average A B C
9 Analysis : Graph two lines 1. Your values of H 2 volume (3 data points) 2. Average volumes of H 2 from the class data (3 data points) Conclusion: As the number of moles of H 2 gas increases, the volume of H 2 gas. This is a (direct / indirect) relationship. The data (supports /does not support) the hypothesis. Error Analysis Sources of error (2) How errors influence the results How can we correct for this error
10 Moles of Gas vs. Volume of a Gas As the moles of a gas increase, the volume of the gas increases provided that the temperature and pressure of the gas remains constant. In this lab The independent variable was the. moles of H 2 gas The dependent variable was the. volume of H 2 gas The controlled variables were the temperature and pressure of the gas.
11 Introduction to Pressure Mass = Weight = amount of matter (g) the force that matter exerts due to gravity, Newtons (N) Pressure = the force (or weight) exerted on a given surface area, Pascals (Pa) 1 Pascal = 1 Newton/m 2 or 1 Pa = 1 N/m 2
12 Activity : What pressure do you exert on the ground below your feet? Step 1: Calculate your weight in Newtons. Weight = Force = lbs 454 g = m_ m = g 1000 = kg Multiply the answer by 9.8 m/s 2 to account for the force of gravity on the body. kg X 9.8 m/s 2 = kg.m/s 2 = N = N correct number of significant figures
13 Step 2: What is the contact surface area that your body makes with the ground? Take off your right shoe and place your right foot on a piece of graph paper on the floor. Taking turns, your partner can trace the outline of your foot on the graph paper. Then count the number of square centimeters (surface area) of your foot. Multiply this value by because you have. Surface area = cm 2 = m 2 Step 3: Calculate the pressure you exert on the ground below your feet? Pressure (Pa) = Weight (N) surface area (m 2 ) Pressure (kpa) = Pressure (Pa) 1000
14 Experiment: The Volume and External Pressure of a Gas (Formal Lab Write-up typed or hand written) Problem: What effect does an increase in external pressure have on the volume of a gas? Hypothesis: As the external pressure increases, the volume of a gas will because. Procedure: Look at the syringe set in the wood block. How can you place 1, then 2 and then 3 bricks on top? Does it make any difference how you position the bricks? Discuss and write, with your partner, a procedure
15 This is called Law. Error Analysis Sources of error How errors influence the results How can we correct for this error Diagram: Data: Analysis: Look at the apparatus label the diagram In a table (Observations only) Pressure calculations Graph of your data (Volume (ml) vs. Pressure (kpa) When the pressure doubles the volume. When the pressure halves, the volume. Conclusion: As the external pressure increases, the volume of a gas provided the quantity of gas and the temperature remain constant. This is a (direct /indirect) relationship. The data (supports /does not support) the hypothesis.
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