A student, following the procedure described in this exercise, collected the following data: mass Mg,g .0243...
A student, following the procedure described in this exercise, collected the following data: mass Mg,g .0243 Final gas volume 25.0 barometric pressure, torr 754 Vapor pressure of H2O @ 25degreesC 23.76 Temperature, K 298
*The gas collected in the eidiometer is a mixture of hydrogen gas and water vapor.
Calculate the gas law constant.
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A student, following the procedure described in this exercise,
collected the following data: mass Mg,g .0243...
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...
A student follows the procedure described in the experiment and collected the following data: 25.5 mL...
A student follows the procedure described in the experiment and collected the following data: 25.5 mL of hydrogen gas collected, barometric pressure of 755 mm Hg, and a temperature of 298 K. Use the ideal gas law (PV=nRT) to answer the questions below. The R value is 0.08206 L atm / Kmol and our data must be in these units. The temperature is given in Kelvin, so no conversion is needed. But the hydrogen gas volume and pressure need conversion...
PRORO332 Evaluation of the Gas Law Coestant 69 Dahida Ch Date Pre-Laboratory Assi nt gnme 1....
PRORO332 Evaluation of the Gas Law Coestant 69 Dahida Ch Date Pre-Laboratory Assi nt gnme 1. A student following the procedure described in this module collected the following data: mass Mg,8 initial syringe volume, mL final syringe volume, mL barometric pressure, torr temperature, K 0.0243 1.0 26.5 754 298 Calculate the gas law constant. 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...
A-D A student performed an experiment in which they collected hydrogen gas from the reaction of...
A-D
A student performed an experiment in which they collected hydrogen gas from the reaction of magnesium with hydrochloric acid using the same apparatus that you will be using in today's lab. The reaction is: Mg(s) + 2 HCl(aq) → H2(g) + MgCl2 (aq) The data they collected are shown below: Mass of Mg Volume of HCI Volume of H2 collected Temperature of H2 collected Barometric pressure 0.100 g 10 mL 57.5 mL 22 °C 29.94 in Hg a. Barometric...
Can you help answer all questions? I dont know how to answer any of the question...
Can you help answer all questions?
I
dont know how to answer any of the question i dont know what kind
of math to use
PROP033: En of the Gul Pre-Laboratory Assignment 1. A student following the procedure described in this module collectes procedure described in this module collected the following data 0.0243 10 mass Mg 8 initial syringe volume, mL final syringe volume, ml barometric pressure, torr temperature, K Calculate the gas law constant. 26.5 754 298 answer 2....
9. A student collected the following data: Mass of gas = 0.800 g, temperature of the...
9. A student collected the following data: Mass of gas = 0.800 g, temperature of the water bath = 95.0°C, barometric pressure = 760.0 torr, and the volume of the flask = 250.0 mL. Later the student was told that one drop (0.050g) of water had been present in the flask during the experiment and it completely vaporized, contaminating the gas. (a) Calculate the apparent molar mass, that is, the molar mass the student would get if he did not...
A student performed an experiment in which hydrogen gas was collected over water from the reaction...
A student performed an experiment in which hydrogen gas was collected over water from the reaction of magnesium and hydrochloric acid using the apparatus shown and accoridng to the reaction equation and the data collected shown below: Mass of Mg 0.100 g Volume of HCl 10 mL Volume of H2 collected 57.5 mL Temperature of H2 collected 22.0 oC Barometric pressure 29.94 inHg Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) a. Barometric pressure in atmospheres? b. Water vapor pressure...
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the...
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 96.96 mL Temperature 25.0°C Barometric pressure 742 mmHg Vapor pressure of water at 25.0°C 24.0 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: mol H2
hydrogen produced from a hydrolysis reaction was collected overwater the data is complied in the table...
hydrogen produced from a hydrolysis reaction was collected overwater the data is complied in the table total volume of H2(g) collected = 96.41 mL temperature = 25.0 C Barometric pressure = 742 mmHg Vapor pressure of water at 25.0 C = 24.0 mmHg calculate the moles of hydrogen gas produced by the reaction
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...
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...
PRORO332 Evaluation of the Gas Law Coestant 69 Dahida Ch Date Pre-Laboratory Assi nt gnme 1. A student following the procedure described in this module collected the following data: mass Mg,8 initial syringe volume, mL final syringe volume, mL barometric pressure, torr temperature, K 0.0243 1.0 26.5 754 298 Calculate the gas law constant. 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...
A-D
A student performed an experiment in which they collected hydrogen gas from the reaction of magnesium with hydrochloric acid using the same apparatus that you will be using in today's lab. The reaction is: Mg(s) + 2 HCl(aq) → H2(g) + MgCl2 (aq) The data they collected are shown below: Mass of Mg Volume of HCI Volume of H2 collected Temperature of H2 collected Barometric pressure 0.100 g 10 mL 57.5 mL 22 °C 29.94 in Hg a. Barometric...
Can you help answer all questions?
I
dont know how to answer any of the question i dont know what kind
of math to use
PROP033: En of the Gul Pre-Laboratory Assignment 1. A student following the procedure described in this module collectes procedure described in this module collected the following data 0.0243 10 mass Mg 8 initial syringe volume, mL final syringe volume, ml barometric pressure, torr temperature, K Calculate the gas law constant. 26.5 754 298 answer 2....
9. A student collected the following data: Mass of gas = 0.800 g, temperature of the water bath = 95.0°C, barometric pressure = 760.0 torr, and the volume of the flask = 250.0 mL. Later the student was told that one drop (0.050g) of water had been present in the flask during the experiment and it completely vaporized, contaminating the gas. (a) Calculate the apparent molar mass, that is, the molar mass the student would get if he did not...
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 96.96 mL Temperature 25.0°C Barometric pressure 742 mmHg Vapor pressure of water at 25.0°C 24.0 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: mol H2
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