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Experiment is done at the following conditions. Temperature of boiling water (°C) 99.2 Atmoshperic Pressure (torr)...
Experiment is done at the following conditions Temperature of boiling water (C) 99.8 1755 Atmoshperic Pressure...
Experiment is done at the following conditions Temperature of boiling water (C) 99.8 1755 Atmoshperic Pressure (torr) Results Trial Trial 2 Trial 3 Volume of flask (ml) 141.62 141.62 75.649 Mass of dry flask, foil, and rubber band (9) 75.655 141.62 75.653 75.865 0.212 75.868 Mass of flask, foil, rubber band and vapor (@) 75.864 Mass of vapor (9) 0.215 Calculations 0.212 2 M Unknown number Number of moles using ideal gas law g/mol) Molar mass using ideal gas law...
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of wat...
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of water bath (°C) 100t 99.1 Mass of Erlenmeyer flask, rubber band, foil cover and condensed 0819 gas sample (9) Mass of the condensed gas sample (9) 251.59 Barometric (atmospheric) pressure (mmHg) 128.96 28.93 Volume of the Erlenmeyer flask (mL) 170 170 Molar mass of the unknown sample (g/mole) Average molar mass (g/mol): DATA ANALYSIS (Show your calculations) 1. Determine the...
can anyone show me how to find M Temperature of boiling water bath Mass of flask...
can anyone show me how to find M
Temperature of boiling water bath Mass of flask + rubber band + foil + condensed gas Mass of flask + rubber band + foil 1ST TRIAL 2ND TRIAL 100.5 °C 100.5 °C 123,713 8 123.452 8 123.351g 103.452 8 16.3628 0.756 8 373.5 k 375.5 0.0821 L'atm/molek Mass of condensed gas Temperature of vapor (converted to K) Universal gas constant, R Barometric Pressure (converted to atm) atm a9986 0.0663 Volume of flask...
need help on part B a Calculate the pressure exerted by 20.0 g of Co, in...
need help on part B
a Calculate the pressure exerted by 20.0 g of Co, in a 600 ml. vessel at 298 K using the ideal gas equation. Then, recalculate the pressure using the van der Waals equation. Assuming that the pressure calculated from the van der Waals equation is correct, what is the percent error in the answer when using the ideal gas equation? Van der Waals constants for CO2 are: a = 3.50 -, and b=0.0427 L/mol; R...
Calculate the pressure exerted by 18.0 g of N2 in a 700. mL vessel at 298...
Calculate the pressure exerted by 18.0 g of N2 in a 700. mL vessel at 298 K using the ideal gas equation. Then, recalculate the pressure using the van der Waals equation. Assuming that the pressure calculated from the van der Waals equation is correct, what is the percent error in the answer when using the ideal gas equation? Van der Waals constants for N2 are: a= 1.39 atm*L^2/mol^2 , and b=0.0391 L/mol ; R=0.082057 L*atm/K*mol. Pideal gas law =...
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p
The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table...
How do you solve Part D. Calculations (Moles of vapor, mass of vapor, and molar mass...
How do you solve Part D.
Calculations (Moles of vapor, mass of vapor, and molar mass of
vapor)
3. a. The following data were recorded in determining the molar mass of a volatile liquid following the Experimental Procedure of this experiment. Complete the table for analysis. (See Report Sheet.) Record calculated values with the correct number of significant figures. Calculation Zone 74.722 Part D.1 98.7 74.921_ Part D.2 A. Preparing the Sample 1. Mass of dry flask, foil, and rubber...
Give the gas you are assigned here And give your temperature and pressure And the number...
Give the gas you are assigned here And give your temperature and pressure And the number of moles Calculate volume of your gas assuming it is ideal. Now calculate volume of your gas assuming it follows the van der Waals equation and using your gas's van der Waals constants from fable 5.4 on page 237 of the textbook.
Barometric Pressure 0.992 atm Mass of Flask + Foil 56 g Mass of Flask + Foil...
Barometric Pressure 0.992 atm Mass of Flask + Foil 56 g Mass of Flask + Foil + Condensed Liquid 59 g Mass of Condensed Liquid 3 g Volume of Flask 300 ml Temperature of Water Bath when Vaporization Begins 333 K Temperature of Water Bath when Water Begins to Boil 363 K Molar Mass 46 g mol Ideal gas law PV=nRT P=pressure V=volume of gas n=number of moles R=gas constant T=temperature Molar volume V=RT/P Density of gas D=PM x RT Molar mass M=(mRT)/(PV) I...
please help. #89 and #101 please nc acid, formic acid decomposes to give CO gas HCHO,)H,O0...
please help. #89 and #101 please
nc acid, formic acid decomposes to give CO gas HCHO,)H,O0 + CO(g) van der Waals Equation If 3.85 L of carbon monoxide was collected over water 5.101 Calculate the pressure of ethanol vapor, C,H2OH(g), at 82.0°C if 1.000 mol C>H OH(g) occupies 30.00 L. Use the van der Waals equation (see Table 5.7 for data). Com- pare with the result from the ideal gas law. 5.102 Calculate the pressure of water vapor at 120.0°C...
Experiment is done at the following conditions Temperature of boiling water (C) 99.8 1755 Atmoshperic Pressure (torr) Results Trial Trial 2 Trial 3 Volume of flask (ml) 141.62 141.62 75.649 Mass of dry flask, foil, and rubber band (9) 75.655 141.62 75.653 75.865 0.212 75.868 Mass of flask, foil, rubber band and vapor (@) 75.864 Mass of vapor (9) 0.215 Calculations 0.212 2 M Unknown number Number of moles using ideal gas law g/mol) Molar mass using ideal gas law...
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of water bath (°C) 100t 99.1 Mass of Erlenmeyer flask, rubber band, foil cover and condensed 0819 gas sample (9) Mass of the condensed gas sample (9) 251.59 Barometric (atmospheric) pressure (mmHg) 128.96 28.93 Volume of the Erlenmeyer flask (mL) 170 170 Molar mass of the unknown sample (g/mole) Average molar mass (g/mol): DATA ANALYSIS (Show your calculations) 1. Determine the...
can anyone show me how to find M
Temperature of boiling water bath Mass of flask + rubber band + foil + condensed gas Mass of flask + rubber band + foil 1ST TRIAL 2ND TRIAL 100.5 °C 100.5 °C 123,713 8 123.452 8 123.351g 103.452 8 16.3628 0.756 8 373.5 k 375.5 0.0821 L'atm/molek Mass of condensed gas Temperature of vapor (converted to K) Universal gas constant, R Barometric Pressure (converted to atm) atm a9986 0.0663 Volume of flask...
need help on part B
a Calculate the pressure exerted by 20.0 g of Co, in a 600 ml. vessel at 298 K using the ideal gas equation. Then, recalculate the pressure using the van der Waals equation. Assuming that the pressure calculated from the van der Waals equation is correct, what is the percent error in the answer when using the ideal gas equation? Van der Waals constants for CO2 are: a = 3.50 -, and b=0.0427 L/mol; R...
How do you solve Part D.
Calculations (Moles of vapor, mass of vapor, and molar mass of
vapor)
3. a. The following data were recorded in determining the molar mass of a volatile liquid following the Experimental Procedure of this experiment. Complete the table for analysis. (See Report Sheet.) Record calculated values with the correct number of significant figures. Calculation Zone 74.722 Part D.1 98.7 74.921_ Part D.2 A. Preparing the Sample 1. Mass of dry flask, foil, and rubber...
Give the gas you are assigned here And give your temperature and pressure And the number of moles Calculate volume of your gas assuming it is ideal. Now calculate volume of your gas assuming it follows the van der Waals equation and using your gas's van der Waals constants from fable 5.4 on page 237 of the textbook.
please help. #89 and #101 please
nc acid, formic acid decomposes to give CO gas HCHO,)H,O0 + CO(g) van der Waals Equation If 3.85 L of carbon monoxide was collected over water 5.101 Calculate the pressure of ethanol vapor, C,H2OH(g), at 82.0°C if 1.000 mol C>H OH(g) occupies 30.00 L. Use the van der Waals equation (see Table 5.7 for data). Com- pare with the result from the ideal gas law. 5.102 Calculate the pressure of water vapor at 120.0°C...
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