A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density o...

Question

Question

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 m

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

from the data Barometric pressure = 30.02 in. Hg. we know that 1 inch of mercury = 25.4 Torr : 25.4 torr 0 x 30:02 in Hg = 1

Add a comment

Answer 2

Similar Homework Help Questions

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...

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 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 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 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
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...

(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
(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
The experiment described in the procedure was performed using a sample of Zinc with HCl(aq). The...

The experiment described in the procedure was performed using a sample of Zinc with HCl(aq). The lab conditions were 27.00°C, and 731.0 torr barometric pressure. 149.0 mg of Zinc (MM: 65.39 g/mol) was reacted with 20.00 mL of 1.00M HCl(aq). 63.049g of water was collected when the reaction was complete, and it required 20.48mL of 0.7500M NaOH(aq) to titrate the reaction mixture. Water at 27.00°C has a density of 0.9965 g/cm3, and a vapor pressure of 26.80 torr. The value...

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...

A student performed the experiment described in this module, using 7.00 mL of a 1.8% H2O2 solution with a density o...

Homework Answers