a student performs this experiment and produces 215 ml of oxygen saturated with water vapor. The...
a student performs this experiment and produces 215 ml of oxygen saturated with water vapor. The temperature is 27 degrees Celsius, atmospheric pressure was 743 mm Hg and the vapor pressure of water at this temperature is 26.7 mmHg. What is the partial pressure of oxygen in this sample? How many moles of oxygen are produced? If the test tube lost 0.258 g of mass during this reaction, what is the molar mass of oxygen?
Homework Answers
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a student performs this experiment and produces 215 ml of oxygen
saturated with water vapor. The...
Hydrogen gas was collected in a tube by water displacement like in your experiment, and adjusted...
Hydrogen gas was collected in a tube by water displacement like in your experiment, and adjusted to have pressure inside the tube equal to atmospheric pressure. If the barometer reads 743 mmHg, and the vapor pressure of water is 3 kPa at today's temperature, what is the partial pressure of hvdmpen in the tube?
A student performs the following experiment : a coffee cup calorimeter contains 50.0g of water at...
A student performs the following experiment : a coffee cup calorimeter contains 50.0g of water at 20.0 degrees Celsius. A student pours an unknown amount of warm water at 55.0 degrees celcius into this cup. The final temperature of the combined water is 34.6 degrees celsius. a. calculate the amount of heat absorbed by the cool water including the sign of q b. calculate the amount of heat released by the WARM water, including the sign of q c. calculate...
You are given an unknown containing KClO3. Following the procedure in your manual, you obtain the...
You are given an unknown containing KClO3. Following the procedure in your manual, you obtain the following fictional data Note! For this problem use the given (allbeit incorrect) vapor pressure of water Mass of empty test tube 71.8394 g Mass of test tube + unknown 72.1363 g Mass of test tube + unknown + MnO2 72.3077 g Mass of erlenmeyer flask with residual water 323.06 g Mass of erlenmeyer flask filled with water 358.52 g Atmospheric pressure 760.9 mmHg Temperature...
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...
Please do the following questions! thank you! Experiment 12: Generating Hydrogen Gas Part B: Molar mass...
Please do the following questions! thank you!
Experiment 12: Generating Hydrogen Gas Part B: Molar mass of unknown metal Unknown #: Mass of unknown metal (X): Volume of H2 gas L K Temperature of H2 gas 0.12588 54.4 mL 23.0 C 765.8 mmHg 21.1 mmHg 744.7 mmHg Atmospheric pressure (see barometer) Vapor pressure of water atm Partial pressure of H, gas Using PV=nRT and your data, calculate the moles of hydrogen gas produced in the experiment: PV = 0.97987x54.4xio RT...
The next three questions go together 21. Expired air is saturated with water vapor and generally...
The next three questions go together 21. Expired air is saturated with water vapor and generally contains more of it than does inspired air. There is usually a net loss of water from the body due to breathing. Water vapor pressure in the at saturation in the lungs (at 37°C) is 47 mmHg, while in expired air at 33°C it is 37.7 mmHg. Consider the case of someone who is breathing dry air in and moist air out at a...
Oxygen gas was collected over hot water at 75 degrees Celsius. A volume of 78.3mL at...
Oxygen gas was collected over hot water at 75 degrees Celsius. A volume of 78.3mL at a total pressure of 101kPa was obtained. The saturated vapour pressure of water at 75 degrees Celsius is 38.7kPa. (i) What was the partial pressure of the oxygen? (ii) What mass of oxygen was collected? (iii) Why was hot water used?
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...
need help to find answers for the blanks Name Chem 2115 Experiment Date Section GAS BEHAVIOR...
need help to find answers for the blanks
Name Chem 2115 Experiment Date Section GAS BEHAVIOR Trial 1 I. Data Mass of test tube and contents 58.726 g 59.601 g before heating 58.619 g 58.726 g afterheating Masa loss 231.8 ml 259.6 mL 25.3 deg C 25.6 deg C 29.79 in Hg Volume of Co, collected, V Temperature of Co,,T Atmospheric pressure Water vapor pressure at Co, temperature 29.80 in Hg IL Calculations Mass of Co, collected Moles of Co,,...
A student performed the experiment described in this module. The 5.00-mL mass of the 2.15% percent...
A student performed the experiment described in this module. The 5.00-mL mass of the 2.15% percent by mass H2O2 solution used was 5.03 g. The water temperature was 230C, and the barometric pressure was 31.2 in. Hg. After the student immersed the yeast in the peroxide solution, she observed a 38.60-mL volume change in system volume. (1) Convert the barometric pressure to torr. (2) Obtain the water vapour pressure at the water temperature. (3) Calculate the pressure, in torr, exerted...
Hydrogen gas was collected in a tube by water displacement like in your experiment, and adjusted to have pressure inside the tube equal to atmospheric pressure. If the barometer reads 743 mmHg, and the vapor pressure of water is 3 kPa at today's temperature, what is the partial pressure of hvdmpen in the tube?
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...
Please do the following questions! thank you!
Experiment 12: Generating Hydrogen Gas Part B: Molar mass of unknown metal Unknown #: Mass of unknown metal (X): Volume of H2 gas L K Temperature of H2 gas 0.12588 54.4 mL 23.0 C 765.8 mmHg 21.1 mmHg 744.7 mmHg Atmospheric pressure (see barometer) Vapor pressure of water atm Partial pressure of H, gas Using PV=nRT and your data, calculate the moles of hydrogen gas produced in the experiment: PV = 0.97987x54.4xio RT...
The next three questions go together 21. Expired air is saturated with water vapor and generally contains more of it than does inspired air. There is usually a net loss of water from the body due to breathing. Water vapor pressure in the at saturation in the lungs (at 37°C) is 47 mmHg, while in expired air at 33°C it is 37.7 mmHg. Consider the case of someone who is breathing dry air in and moist air out at a...
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...
need help to find answers for the blanks
Name Chem 2115 Experiment Date Section GAS BEHAVIOR Trial 1 I. Data Mass of test tube and contents 58.726 g 59.601 g before heating 58.619 g 58.726 g afterheating Masa loss 231.8 ml 259.6 mL 25.3 deg C 25.6 deg C 29.79 in Hg Volume of Co, collected, V Temperature of Co,,T Atmospheric pressure Water vapor pressure at Co, temperature 29.80 in Hg IL Calculations Mass of Co, collected Moles of Co,,...
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