Jennifer Jiang Dr. Iobst Chemistry I Honors 11 March 2013 Molar Mass of Butane: Applying the Gas Laws 1. Water bath temperature: 17.7° C or 291 K Celsius to Kelvin temperature conversion: 17.7° C + 273 = 290.7 Kelvin (rounded to SF= 291 K) 2. 1 atm 1 atm 10 mm 10 mm 2.54 cm 2.54 cm According to the digital barometer our teacher provided‚ the barometric pressure in the lab is 29.77 in Hg‚ which will need to be converted to atmospheric pressure. 760 mm Hg 760 mm Hg 1 cm
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Physics Practical Report: Experiment: Ohmic Resistance and Ohm’s Law Patrick Doan Mr Sadowsky 11 PHYS 71 12/9/08 Table of contents 1.0 Aim 1 2.0 Hypothesis 1 3.0 Materials 1 4.0 Method 2 5.0 Results 3 - 5.1 Qualitative Observations 3 - 5.2 Data 3-4 6.0 Discussion 5 7.0 Conclusion 6 8.0 Bibliography 7 9.0 Acknowledgements 7 1.0 Aim: To find out how current‚ voltage and resistance in a circuit
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Experiment 11 The Gas Laws Introduction: In this experiment you will (1) determine whether Boyle’s Law applies to a mixture of gases (air) and (2) calculate the gas constant‚ R‚ by determining the volume of a known amount of gas (H2) at a measured temperature and pressure. Determination of Whether Boyle’s Law Applies to Air Boyle’s Law states that for a fixed amount of gas at constant temperature‚ the pressure of the gas will vary inversely with the volume so that P ∝ 1/V or PV = a constant (if
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S74 assignment Introduction Sir Isaac Newton’s second law describes how the mass of an object changes the way that it moves when acted upon (Jacplus 2013). This means that the more mass that an object has‚ the harder it will be to move. Mass can be calculated using the formula: F=ma * Where: F is the force (N) * m is the mass (kg) * a is the acceleration (m/s/s) If there are two balls and one has a mass of 1kg and the other has a mass of 2kg‚ then the ball that has a larger mass
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___________________________ 14.3 Date ___________________ Class __________________ IDEAL GASES Section Review Objectives • Compute the value of an unknown using the ideal gas law • Compare and contrast real and ideal gases Vocabulary • ideal gas constant (R) • ideal gas law Key Equation • Ideal gas law: P V n R T or PV nRT Part A Completion © Pearson Education‚ Inc.‚ publishing as Pearson Prentice Hall. All rights reserved. Use this completion exercise to
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The Gas Laws The Gas Laws 1. Boyle’s Law – P-V Relationship the pressure of a fixed amount of gas maintained at constant temperature is inversely proportional to the volume of the gas. The Gas Laws 2. Charles’ Law – T-V Relationship the volume of a fixed amount of gas maintained at constant pressure is directly proportional to absolute temperature of the gas. The Gas Laws 3. Gay-Lussac’s Law – P-T Relationship the pressure of a fixed amount of gas maintained
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Contents ------------------------------------------------------------------------ I. Introduction………………………………………......3 II. Thermodynamics Properties………...….……………5 III. Thermodynamic Laws……………………………….6 IV. Compression Cycles…………………………………7 V. Ideal Positive Displacement Compressor Cycle……………8 VI. Ideal Dynamic Compressor Cycle.......………………9 VII. Compressor Types……………………………...……9 VIII. Centrifugal Compressor……………………...….…..9 IX
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der Waals forces and relate it to the dipole moment and polarizability of a molecule • Define a potential function • Write equations for ideal gas‚ hard sphere‚ Sutherland‚ and Lennard-Jones potentials and relate them to intermolecular interactions • Explain the origin of an use "complex" equations of state ◦ State the molecular assumptions of the ideal gas law ◦ Explain how the terms in the van der Waals equation relax these assumptions ◦ Describe how cubic equations of state account for attractive
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reaction conducted in this lab‚ including appropriate phase symbols. Mg(s) + 2HCl(aq) --> H2(g) + MgCl2(aq) 2. Determine the partial pressure of the hydrogen gas collected in the gas collection tube. The partial pressure of the hydrogen gas is 1.07 atm 3. Calculate the moles of hydrogen gas collected. pv=mrt ; n= .0013mol of hydrogen gas 4. If magnesium was the limiting reactant in this lab‚ calculate the theoretical yield of the gaseous product. Show all steps of your calculation. 0.03184 g
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Hooke’s Law Lab Report Please complete the following tables and questions and submit them on Blackboard. Observations Data Table 1. Force (N) Top position of spring‚ cm Bottom position of spring‚ cm Elongation‚ cm Bottom reading – top reading Data Point 1 .8 4 5 1 6Data Point 2 1.3 4 6 2 Data Point 3 1.5 4 7 3 Data Point 4 2 4 8 4 Data Point 5 2.2 4 9 5 Data Point 6 2.5 4 10 6 Data Point 7 2.7 4 11 7 Data Point 8 3 4 12 8 Data Point 9 3.3 4 13 9 Data Point 10 3.6 4 14 10 Data Table 2.
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