(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
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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
(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
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 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, 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 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...
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. 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 through E please 5. Last week, a quality control technician for Global Hydrogen Peroxide determined...
A
through E please
5. Last week, a quality control technician for Global Hydrogen Peroxide determined the concentration of a batch of household hydrogen peroxide. She followed the instructions in the Laboratory Investigations section of this experiment and obtained this data: volume of hydrogen peroxide, mL barometric pressure, in. Hg temperature of water, °C volume of oxygen gas collected, mL 8.72 30.09 21.4 99.4 (a) What is the pressure, in atmospheres, of oxygen gas collected? STO10906: Determining Hydrogen peroxide Content...
Following experimental values: Room temp: 295K Barometric pressure: 762.5mmHg vapor pressure: 19.8mmHg Volume O2 collected: 62mL...
Following experimental values: Room temp: 295K Barometric pressure: 762.5mmHg vapor pressure: 19.8mmHg Volume O2 collected: 62mL Density of H2O2: 1.01g/mL % composition of H2O2: 3.02% Volume H202: 5mL Letter of unknown solution of H2O2: c Volume of O2 collected: 56mL 1. Calculate the volume of O2 at STP. 2. Based on the reaction stoichiometry, calculate the number of moles of O2 3. Calculate the mass of O2: 4. Calculate molar volume at STP 5. Calculate the % error of the...
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
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
through E please
5. Last week, a quality control technician for Global Hydrogen Peroxide determined the concentration of a batch of household hydrogen peroxide. She followed the instructions in the Laboratory Investigations section of this experiment and obtained this data: volume of hydrogen peroxide, mL barometric pressure, in. Hg temperature of water, °C volume of oxygen gas collected, mL 8.72 30.09 21.4 99.4 (a) What is the pressure, in atmospheres, of oxygen gas collected? STO10906: Determining Hydrogen peroxide Content...
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