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Student Name Course/Section Date Instructor PRE-LAB ASSIGNMENT 1. A sample of an unknown liquid is vaporized...
Molecular Mass of a Volatile Liquid 1. The atmospheric pressure of a hot summer day in...
Molecular Mass of a Volatile Liquid 1. The atmospheric pressure of a hot summer day in NYC is 29.94 inHg. Calculate this value in mmile and am 2. The atmospheric pressure of a cold winter day in NYC is 25.94 inHg. Calculate this value in Pa. 3. We set up an experiment utilizing the Dumas method to calculate the molar mass of an unknown chemical. A 4.00 mL pure liquid sample of this chemical is vaporized in an Erlenmeyer flask...
Instructor Name: Student Name: DATA (EXP #13): Part 1: The Action of Atmospheric Pressure Observa...
i
need part 2 and part 3 to be solved thanks please please urgent
Instructor Name: Student Name: DATA (EXP #13): Part 1: The Action of Atmospheric Pressure Observations upon immersing the can in ice-water bath: Part 2: Determination of the Molar Mass of Gases Barometric pressure (mmHg): 734.2 mm Room temperature (0 23, 6"c CO2 Natural Gas Mass of flask/stopper filled with air (g) 126 069 125.959 la 0146-16 146.9 Volume of water used to fill flask (mL) 267-nL...
Post Lab #1 A student was assigned the task of determining the molar mass of an unknown gas. The student measured t...
Post Lab #1 A student was assigned the task of determining the molar mass of an unknown gas. The student measured the mass of a sealed 843 mL rigid flask that contained dry air. The student then flushed the flask with the unknown gas, resealed it, and measured the mass again. Both the air and the unknown gas were at 23.0°C and 750. torr. The data for the experiment are shown in the table below. Volume of sealed flask 843...
THE MOLAR MASS OF A VOLATILE LIQUID 1. A foil-covered flask was found to have a...
THE MOLAR MASS OF A VOLATILE LIQUID 1. A foil-covered flask was found to have a mass of 161.38 have a mass of 167.38 g. A volatile liquid was placed L00.0°C at a barometric pressure of 743.8 mm Hg. The foil-covered inside and heated to 100.0°C at a barometric press flask containing the vapor had a mass the molar mass of this volatile liquid. 's the vapor had a mass of 167.71 g and a volume of 147.0 mL. Calculate...
please help ? MST SHOW ALL CALCULATIONSs. Please be neat. Use correct significant figures. 1. A...
please help ?
MST SHOW ALL CALCULATIONSs. Please be neat. Use correct significant figures. 1. A student masses an empty flask, aluminum foil (witha small pinhole), and copper wire and finds the mass to be 54.8680 g. She then adds about 5.0 mL of an unknown liquid and heats the flask in a hot waterbath to 95.0 °C. After all the liquid is vaporized, she removes the flask from the bath and masses it after it has cooled. The mass...
PROP0332: Evaluation of the Gas Law Constant Name Section Date Pre-Laboratory Assignment 1. A student following...
PROP0332: Evaluation of the Gas Law Constant Name Section Date Pre-Laboratory Assignment 1. A student following the procedure described in this module collected the following data: 20 mass Mg 8 initial syringe volume, mL final syringe volume, mL barometric pressure, torr temperature, K Calculate the gas law constant. 0.0243 1.0 26.5 754 298 answer 2. What would be the volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298...
i dont understand why the molecular weight i calculated (42.012 g/mol) for my unknown liquid (acetone)...
i dont understand why the molecular weight i calculated
(42.012 g/mol) for my unknown liquid (acetone) is less than the
actual molecular weight (58.08 g/mol). what errors could i have
made in my lab that would account for the difference.
Molecular Weight of a Volatile Liquid In this experiment, an amount of liquid more than sufficient to fill the flask when vaporized is placed in a flask of measured volume and mass. The flask is then heated in a boiling...
Problems Section 1. A 0.678 gram sample of gas occupies 0.214 L at standard conditions, what...
Problems Section 1. A 0.678 gram sample of gas occupies 0.214 L at standard conditions, what is the molar mass of the gas? PronRT 1 (0,214) = NA 273.15 n = R-273.15 n=104,684 -:675 X=18 2. A sample of gas occupies 250 mL at 37°C and 730. torr, what volume would the gas occupy at standard conditions? ,250L 310k 730 + 20.5 10.0206-310 .216L n=0.0094396539 V nr. 273.15 = 2115 3. A 5.00 mL sample of an unknown liquid is...
Name: Date: Instructor's Initials: Lab Section: The Ideal Gas Constant PreLab: sing the Balanced Equation (1),...
Name: Date: Instructor's Initials: Lab Section: The Ideal Gas Constant PreLab: sing the Balanced Equation (1), determine how many moles of hydrogen should be produced by 0.036 grams of Mg metal using an excess of HCI. If the average temperature of the water was 21.5 °C, what pressure inside the Graduated cylinder is contributed by the water vapor? (See Table 1). 3. If the atmospheric pressure in the lab was 754 mmHg on that day, what would be the pressure...
Can, anyone make sure these answers are correct? 1. If 0.765g of an unknown gas is...
Can, anyone make sure these answers are correct?
1. If 0.765g of an unknown gas is collected at 741 torr (corrected) and 95°C in a 245 ml container, calculate the molecular weight of this unknown gas? P=741 tona PV=ART -> ideal gas equation n=PU T=95C+243=368K BT mass of the gas = 0.7659 =a41tów 80.245€ R= 62-4L-fowl mol- 624kbar V=245 med 'x 36644 Moler mass of the gos= 0.7659 245L 6 +91-1 60079rmal 2. If in the experiment in Question 1,...
Molecular Mass of a Volatile Liquid 1. The atmospheric pressure of a hot summer day in NYC is 29.94 inHg. Calculate this value in mmile and am 2. The atmospheric pressure of a cold winter day in NYC is 25.94 inHg. Calculate this value in Pa. 3. We set up an experiment utilizing the Dumas method to calculate the molar mass of an unknown chemical. A 4.00 mL pure liquid sample of this chemical is vaporized in an Erlenmeyer flask...
i
need part 2 and part 3 to be solved thanks please please urgent
Instructor Name: Student Name: DATA (EXP #13): Part 1: The Action of Atmospheric Pressure Observations upon immersing the can in ice-water bath: Part 2: Determination of the Molar Mass of Gases Barometric pressure (mmHg): 734.2 mm Room temperature (0 23, 6"c CO2 Natural Gas Mass of flask/stopper filled with air (g) 126 069 125.959 la 0146-16 146.9 Volume of water used to fill flask (mL) 267-nL...
Post Lab #1 A student was assigned the task of determining the molar mass of an unknown gas. The student measured the mass of a sealed 843 mL rigid flask that contained dry air. The student then flushed the flask with the unknown gas, resealed it, and measured the mass again. Both the air and the unknown gas were at 23.0°C and 750. torr. The data for the experiment are shown in the table below. Volume of sealed flask 843...
THE MOLAR MASS OF A VOLATILE LIQUID 1. A foil-covered flask was found to have a mass of 161.38 have a mass of 167.38 g. A volatile liquid was placed L00.0°C at a barometric pressure of 743.8 mm Hg. The foil-covered inside and heated to 100.0°C at a barometric press flask containing the vapor had a mass the molar mass of this volatile liquid. 's the vapor had a mass of 167.71 g and a volume of 147.0 mL. Calculate...
please help ?
MST SHOW ALL CALCULATIONSs. Please be neat. Use correct significant figures. 1. A student masses an empty flask, aluminum foil (witha small pinhole), and copper wire and finds the mass to be 54.8680 g. She then adds about 5.0 mL of an unknown liquid and heats the flask in a hot waterbath to 95.0 °C. After all the liquid is vaporized, she removes the flask from the bath and masses it after it has cooled. The mass...
PROP0332: Evaluation of the Gas Law Constant Name Section Date Pre-Laboratory Assignment 1. A student following the procedure described in this module collected the following data: 20 mass Mg 8 initial syringe volume, mL final syringe volume, mL barometric pressure, torr temperature, K Calculate the gas law constant. 0.0243 1.0 26.5 754 298 answer 2. What would be the volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298...
i dont understand why the molecular weight i calculated
(42.012 g/mol) for my unknown liquid (acetone) is less than the
actual molecular weight (58.08 g/mol). what errors could i have
made in my lab that would account for the difference.
Molecular Weight of a Volatile Liquid In this experiment, an amount of liquid more than sufficient to fill the flask when vaporized is placed in a flask of measured volume and mass. The flask is then heated in a boiling...
Problems Section 1. A 0.678 gram sample of gas occupies 0.214 L at standard conditions, what is the molar mass of the gas? PronRT 1 (0,214) = NA 273.15 n = R-273.15 n=104,684 -:675 X=18 2. A sample of gas occupies 250 mL at 37°C and 730. torr, what volume would the gas occupy at standard conditions? ,250L 310k 730 + 20.5 10.0206-310 .216L n=0.0094396539 V nr. 273.15 = 2115 3. A 5.00 mL sample of an unknown liquid is...
Name: Date: Instructor's Initials: Lab Section: The Ideal Gas Constant PreLab: sing the Balanced Equation (1), determine how many moles of hydrogen should be produced by 0.036 grams of Mg metal using an excess of HCI. If the average temperature of the water was 21.5 °C, what pressure inside the Graduated cylinder is contributed by the water vapor? (See Table 1). 3. If the atmospheric pressure in the lab was 754 mmHg on that day, what would be the pressure...
Can, anyone make sure these answers are correct?
1. If 0.765g of an unknown gas is collected at 741 torr (corrected) and 95°C in a 245 ml container, calculate the molecular weight of this unknown gas? P=741 tona PV=ART -> ideal gas equation n=PU T=95C+243=368K BT mass of the gas = 0.7659 =a41tów 80.245€ R= 62-4L-fowl mol- 624kbar V=245 med 'x 36644 Moler mass of the gos= 0.7659 245L 6 +91-1 60079rmal 2. If in the experiment in Question 1,...
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