A student performed the experiment described in this module, using 5.00 mL of a 2.50% H2O2 solution with a density of 1.01 g mL-1
2. A student performed the experiment described in this module, using 5.00 mL of a 2.50% H2O2 solution with a density of 1.01 g mL-1. The water temperature was 24°C, and the barometric pressure in the labora- tory was 30.50 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 43.70 mL of O2.
(8) Calculate the number of moles of H2O2 reacting
(9) Calculate the number of moles of collected O2
(10) Calculate the molar volume of O2 at STP.
(11) Calculate the percent error for the experiment.
Homework Answers
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A student performed the experiment described in this module, using 5.00 mL of a 2.50% H2O2 solution with a density of 1.01 g mL-1
A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density o...
A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density of 1.01 g ml-1. The water temperature was 20 °C, and the barometric pressure in the laboratory was 30.02 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 45.1 ml of 02. (8) Calculate the number of moles of H2O2 reacting.
A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density o...
A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density of 1.01 g ml-1. The water temperature was 20 °C, and the barometric pressure in the laboratory was 30.02 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 45.1 ml of Oz. (1) Convert the barometric pressure to torr.
A student performed the experiment described in this module, using 4.00 mL of a 3.5% H2O2...
A student performed the experiment described in this module, using 4.00 mL of a 3.5% H2O2 solution with a density of 1.61 g ml-1. The water temperature was 25 °C, and the barometric pressure in the laboratory was 30.40 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 79.20 mL of O2. (5) Convert the volume, in liters, that the collected O2 would occupy at STP.
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...
A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2...
A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density of 1.01 g ml-1. The water temperature was 20 °C, and the barometric pressure in the laboratory was 30.02 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 45.1 mL of Oz. (2) Obtain the water vapor pressure at the water temperature, Answer: Check
A student performed the experiment described in this module, using 6.00 mL of a 3% H202...
A student performed the experiment described in this module, using 6.00 mL of a 3% H202 solution with a density of 1.03 g mL-1. The water temperature was 22 C, and the barometric pressure in the laboratory was 30.30 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 65.40 ml of O2 (4) Calculate the water temperature, in Celsius, to kelvins
(9) Calculate the number of moles of collected O2
A student performed the experiment described in this module, using 6.00 mL of a 3% H2O2 solution with a density of 1.03 g ml-1. The water temperature was 22 °C, and the barometric pressure in the laboratory was 30.30 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 65.40 mL of O2. (9) Calculate the number of moles of collected O2
(3) Calculate the pressure, in torr, exerted by the collected O2 at the water temperature
A student performed the experiment described in this module, using 4.00 mL of a 3.5% H2O2 solution with a density of 1.61g mL-1. The water temperature was 25℃, and the barometric pressure in the laboratory was 30.40 in. Hq. After the student immersed the yeast in the peroxide solution, she collected 79.20 mL of O2 (3) Calculate the pressure, in torr, exerted by the collected O2 at the water temperature
Given: Room temperature: 293.0 K Barometric pressure: 764.0 mmHg Vapor of water: 17.5 mmHg Volume of...
Given: Room temperature: 293.0 K Barometric pressure: 764.0 mmHg Vapor of water: 17.5 mmHg Volume of O2 collected: 68.00 mL Density of H2O2: 1.01 g/mL % Composition H2O2: 3.02 % Volume of H2O2 used: 5.00 mL Letter of the unknown solution of H2O2: A Volume of O2 collected for the unknown: 43.00 mL Calculate the corrected barometric pressure. (mmHg) Calculate the volume of O2 at STP. (mL) Based on the reaction stoichiometry, calculate the number of moles of O2. (moles)...
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...
A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density of 1.01 g ml-1. The water temperature was 20 °C, and the barometric pressure in the laboratory was 30.02 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 45.1 ml of 02. (8) Calculate the number of moles of H2O2 reacting.
A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density of 1.01 g ml-1. The water temperature was 20 °C, and the barometric pressure in the laboratory was 30.02 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 45.1 ml of Oz. (1) Convert the barometric pressure to torr.
A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density of 1.01 g ml-1. The water temperature was 20 °C, and the barometric pressure in the laboratory was 30.02 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 45.1 mL of Oz. (2) Obtain the water vapor pressure at the water temperature, Answer: Check
A student performed the experiment described in this module, using 6.00 mL of a 3% H202 solution with a density of 1.03 g mL-1. The water temperature was 22 C, and the barometric pressure in the laboratory was 30.30 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 65.40 ml of O2 (4) Calculate the water temperature, in Celsius, to kelvins
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