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What is the molar mass of a 0.199-g sample of an unknown (ideal gas occupying a...
O GASES Christ Interconverting molar mass and density of ideal gases A sample of an unknown...
O GASES Christ Interconverting molar mass and density of ideal gases A sample of an unknown compound is vaporized at 190. °C. The gas produced has a volume of 2130. mL at a pressure of 1.00 atm, and it weighs 1.80 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. mol
12. Compute the molar mass of an unknown pure ideal gas if 3.88 g sample of...
12. Compute the molar mass of an unknown pure ideal gas if 3.88 g sample of the gas exerts a pressure of 0.524 atm at 25.1 °C in a container of 4.75 L in volume.
A sample of N2 gas is contaminated with a gas (A) of unknown molar mass. The...
A sample of N2 gas is contaminated with a gas (A) of unknown molar mass. The partial pressure of each gas is known to be 200. torr at 25°C. The gases are allowed to effuse through a pinhole, and it is found that gas A escapes at 2 times the rate of N2. The molar mass of gas A is: 56 g/mol 14.01 g/mol 7.00 g/mol 112 g/mol none of these
1. A 125mL Erlenmeyer flask has a measure volume of 152 mL. A 0.177 g sample...
1. A 125mL Erlenmeyer flask has a measure volume of 152 mL. A 0.177 g sample of an unknown vapor occupies the flask at 97.8°C a pressure of 748 torr. Assume ideal gas behavior. a. How many moles of vapor are present? b. What is the molar mass of the vapor? 2. a) If the volume of the flask is mistakenly recorded as 125mL in Question 1, what is the reported molar mass of the vapor? b) What is the...
O GASES Interconverting molar mass and density of Ideal gases A sample of an unknown compound...
O GASES Interconverting molar mass and density of Ideal gases A sample of an unknown compound is vaporized at 110 °C. The gas produced has a volume of 1070. ml. at a pressure of 1.00 atm, and it weighs 1.72 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. 1xlml?
Question 10 of 22 A 4.05 g sample of an unknown gas at 35 °C and...
Question 10 of 22 A 4.05 g sample of an unknown gas at 35 °C and 1.05 atm is stored in a 2.15 L flask. What is the density of the gas? density: 1.88372 g/L What is the molar mass of the gas? molar mass: g/mol Incorrect Question 14 of 22 A gas mixture is made by combining 6.7 g each of Ar, Ne, and an unknown diatomic gas. At STP, the mixture occupies a volume of 15.14 L. What...
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...
What is the molar mass of an ideal gas if a 0.72 g sample of this...
What is the molar mass of an ideal gas if a 0.72 g sample of this gas occupies a volume of 475./. mat 50.0°C and 720. mm Hg? Flag question Select one: O a. 42.40 g/mol O b. 16.98 g/mol c. 660.69 g/mol O d. 1.51 g/mol Oe. 20.17 g/mol son 8 Consider the following reaction: 2Al(s) + 3Cl2(g) - 2AlCl3(s), AH = -1391 kJHow many moles of Al are required to releasee 714.3 kJ of energy (assume 100% yield)...
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...
Experiment 12: Generating Hydrogen Gas Part B: Molar mass of unknown metal Unknown #: Mass of...
Experiment 12: Generating Hydrogen Gas Part B: Molar mass of unknown metal Unknown #: Mass of unknown metal (X) .29 Volume of H2 gas L mL Temperature of H; gas 20 mm к C Atmospheric pressure (see barometer) Vapor pressure of water mmHg Partial pressure of H; gas mmHg atm Using PV-nRT and your data, calculate the moles of hydrogen gas produced in the experiment: l e epl8 moles H Convert moles of hydrogen gas to moles of the metal...
O GASES Christ Interconverting molar mass and density of ideal gases A sample of an unknown compound is vaporized at 190. °C. The gas produced has a volume of 2130. mL at a pressure of 1.00 atm, and it weighs 1.80 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. mol
12. Compute the molar mass of an unknown pure ideal gas if 3.88 g sample of the gas exerts a pressure of 0.524 atm at 25.1 °C in a container of 4.75 L in volume.
1. A 125mL Erlenmeyer flask has a measure volume of 152 mL. A 0.177 g sample of an unknown vapor occupies the flask at 97.8°C a pressure of 748 torr. Assume ideal gas behavior. a. How many moles of vapor are present? b. What is the molar mass of the vapor? 2. a) If the volume of the flask is mistakenly recorded as 125mL in Question 1, what is the reported molar mass of the vapor? b) What is the...
O GASES Interconverting molar mass and density of Ideal gases A sample of an unknown compound is vaporized at 110 °C. The gas produced has a volume of 1070. ml. at a pressure of 1.00 atm, and it weighs 1.72 g. Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. 1xlml?
Question 10 of 22 A 4.05 g sample of an unknown gas at 35 °C and 1.05 atm is stored in a 2.15 L flask. What is the density of the gas? density: 1.88372 g/L What is the molar mass of the gas? molar mass: g/mol Incorrect Question 14 of 22 A gas mixture is made by combining 6.7 g each of Ar, Ne, and an unknown diatomic gas. At STP, the mixture occupies a volume of 15.14 L. What...
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...
What is the molar mass of an ideal gas if a 0.72 g sample of this gas occupies a volume of 475./. mat 50.0°C and 720. mm Hg? Flag question Select one: O a. 42.40 g/mol O b. 16.98 g/mol c. 660.69 g/mol O d. 1.51 g/mol Oe. 20.17 g/mol son 8 Consider the following reaction: 2Al(s) + 3Cl2(g) - 2AlCl3(s), AH = -1391 kJHow many moles of Al are required to releasee 714.3 kJ of energy (assume 100% yield)...
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...
Experiment 12: Generating Hydrogen Gas Part B: Molar mass of unknown metal Unknown #: Mass of unknown metal (X) .29 Volume of H2 gas L mL Temperature of H; gas 20 mm к C Atmospheric pressure (see barometer) Vapor pressure of water mmHg Partial pressure of H; gas mmHg atm Using PV-nRT and your data, calculate the moles of hydrogen gas produced in the experiment: l e epl8 moles H Convert moles of hydrogen gas to moles of the metal...
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