Physics II Lab 1 Report

Part IV:  Relationships Between Gas Variables   Scientists in the late 1800’s noted relationships between many of the state variables related to gases (pressure, volume, temperature), and the number of gas particles in the sample being studied.  They knew that it was easier to study relationships if they varied only two parameters at a time and “fixed” (held constant) the others.  Use the simulation (PhET) to explore these relationships.   Variables Constant Parameters Relationship Proportionality (see hint below) pressure, volume Pressure- 11.8 atm Particle- 100 Inversely proportional directly proportional or inversely proportional volume, temperature     directly proportional or inversely proportional volume, number of gas particles     directly proportional or inversely proportional   Hint: A pair of variables is directly proportional when they vary in the same way (one increases and the other also increases).  A pair of variables is…

Part IV:  Relationships Between Gas Variables   Scientists in the late 1800’s noted relationships between many of the state variables related to gases (pressure, volume, temperature), and the number of gas particles in the sample being studied.  They knew that it was easier to study relationships if they varied only two parameters at a time and “fixed” (held constant) the others.  Use the simulation to explore these relationships.   Variables Constant Parameters Relationship Proportionality (see hint below) pressure, volume     directly proportional or inversely proportional volume, temperature     directly proportional or inversely proportional volume, number of gas particles     directly proportional or inversely proportional   Hint: A pair of variables is directly proportional when they vary in the same way (one increases and the other also increases).  A pair of variables is inversely proportional when they vary in opposite ways (one…

Applications of physical chemistry to daily life

The model of ideal gases shown above is useful because it  _______.  a: helps us understand nonideal gas behavior. b: predicts the behavior of other phases of matter. c: shows a linear relation between gas pressure and volume. a: accurately approximates the properties of most gas molecules.

Not for a grade!!!

BIOL 1603: Org & Evol - Google x A ALEKS - Katie Matthews - Grac x Content app.101edu.co → C esc 1 F1 A glass container was initially charged with 1.50 moles of a gas sample at 5.00 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 33.1 °C, so the final pressure in the container was reduced to 1.50 atm. How many moles of the gas sample are present at the end? Q 2 F2 W # 3 80 E $ 4 F4 R % 675 뽀 F5 T 6 X Question 38 of 66 F6 Y Aktiv Chemistry & 7 F7 U * 00 8 DII F8 ( 1 9 X a Amazon.com: wireles F9 0 1 2 4 7 +/- 0 7 F10 5 8 P

1. Prove that 1 L = 1 x 19-3 m3 2. Calculate the number of moles of an ideal gas given the following: P = 743.3 Torr; V = 262.84 mL; T= 100°C; R = 8.314 Pa-m3 / mol·K (HINT: Use Ideal Gas equation (PV = nRT) and SI Units. %3D 3. Plot the following using MS Excel: a) Volume (mL) vs Pressure (kPa) b) 1/volume vs Pressure Given the following data: V (mL) P (kPa) 15 16 14 12 10 8 6 100 95 105 118 131 139 180

Does the data from my lab verify Boyles law? Please explain

10-53 A diver, originally 20 m below the sur- face, ascends, expelling air as she rises to keep her lung volume constant. The air bubbles rise faster than she does. If her lung volume is 2.4 litres, what is the total volume of expelled air in the bubbles at the water surface? (The pressure changes by l'atm for each 10.3 m of depth change in water)

we use Pv=nRT. Everything here should be related to H2 (g)    --> Chemical equation1Mg +2 HCl à MgCl2 +H2(g) From video : mass of Mg =.0407 g H2 gas volume = 38.2ml Temperature of room=24.0 +273=297k Total Pressure of the room = 30.01 in mmHg Calculations: find total pressure from barometer and convert it to mmHg, 1 in =2.54 cm and 25.4 mm 30.01 in mmHg x 25.4 mm Hg =762.3 mmHg total pressure of room ​    ​​ 1in mmHg  First step- convert g of Mg to mol of H2 0.0407g Mg x 1mol/24 gx 1molH2 = 0.00169mol                                          1mol Mg Second step: Total pressure of gas = Pressure of H2 + P of water 762.3 = p H2 + 22.4    FROM reference (canvas)=Pressure of water at 24 C= 22.4 mmHg n= 0.00169mol H2 Pressure of H2= 762.3-22.4= 739.854  x 1atm/760= 0.973 atm H2 Volume of H2= 38.2 ml /1000 =0.038L H2 Temp= 297K   anwer this quesions with the information provide: Using PV=nRT, Find R=? (No R averge needed)  à 0.973X0.0382=0.00169XRx 297  0.0372=0.50R Then, Percent error…

Please help with question 2 a-c

Part C Calculate the relative difference of the real (van-der- Waals) gas pressure to the ideal gas pressure under these conditions in %. Assume the ideal gas pressure to be 100%. By how many % does the predicted pressure increase (positive answer) or decrease (negative answer) upon the use of the van - der - Waals corrections compared to the ideal gas law? Express your answer as a percentage with 3 significant figures. For carbon dioxide gas (CO₂), the constants in the van der Waals equation 3 3 m are a = 0.364J*ol² and b = 4.27 x 10 -ol. -5m m m For carbon dioxide gas (CO₂), the constants in the van der Waals equation are a 0.364 J-m³/mol and b= 4.27 x 10 m³/mol.

25 a. A chemist collects an unknown gas. Its volume is 0.865L at 17°C and 145 kPa. How many moles of gas are collected? Your answer 25 b. If the mass of the gas is determined to be 0.830 g, what is the molar mass? Your answer 25 c. The chemist believes that the gas could either be CO, CH,, or Cl,. What is the most likely identity of the gas? Your answer

Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H₂(g) collected 95.24 mL Temperature 24.0 °C 739 mmHg 22.5 mmHg Barometric pressure Vapor pressure of water at 24.0 °C Calculate the moles of hydrogen gas produced by the reaction. $ 4 R moles: x10 TOOLS % 5 T G 6 Y MacBook Pro H & 7 U J * 8 - ( 9 K O ) 0 L P mol H₂ + { لالها