Question

In an experiment 158 ml of O2 is collected over water. The mass of the O2...

In an experiment 158 ml of O2 is collected over water. The mass of the O2 is measured to be 0,207g, the temperature is 290k and the barometric pressure that day is 754 mm Hg. Calculate the value of R in the units L, atm, K, mol, showing those units clearly with yoour calculated value. Remember to correct the pressure of O2 for the vapor pressure of water.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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 23 C, 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. (c) Calculate the pressure, in torr, exerted by the collected O2 at the water temperature. (d) Covert this pressue, in torr, to atmospheres....
. A student performed the experiment described in this module, using 5.00 ml of a 2.50%...
. 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 degrees Celsius, and the barometric pressure in the laboratory was 30.50 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 43.70 ml of O2. (A) convert the barometric pressure to torr. (B) Obtain the water vapor pressure at the water temperature. (C) Calculate the pressure,...
2. A student performed the experiment described in this module, using 5.00 ml of a 2.50%...
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 degrees Celsius, and the barometric pressure in the laboratory was 30.50 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 43.70 ml of O2. (A) convert the barometric pressure to torr. (B) Obtain the water vapor pressure at the water temperature. (C) Calculate the pressure,...
Information: In this experiment, you will fill a gelatin capsule with an alloy sample. If the...
Information: In this experiment, you will fill a gelatin capsule with an alloy sample. If the mass of the gelatin capsule is 0.123 g, and the mass of the capsule plus alloy sample is 0.215 g, calculate the mass, in grams, of the alloy sample. - 0.092 g The alloy sample is dissolved in HCl and H2 gas is produced and collected over water. The volume of H2 gas produced is 89.5 mL. What is the volume of gas, in...
Weight of flask and cover 128.7g Weight of flask with vapor 129.4g Pressure of vapor, mm...
Weight of flask and cover 128.7g Weight of flask with vapor 129.4g Pressure of vapor, mm Hg 760 Pressure of, atm 1 Mass of water in flask 250g Temperature of water in flask (boiling water) =92c Temperature of vapor in K= 92C+273=365K Temperature of water in the flask= 25t the volume of vapor in the flask 250 ML Using the volume of the flask (in liters) the temperature of the boiling-water bath (in kelvins), and the barometric pressure (in atmospheres),...
In a laboratory experiment, a student found that a 158-mL aqueous solution containing 2.589 g of...
In a laboratory experiment, a student found that a 158-mL aqueous solution containing 2.589 g of a compound had an osmotic pressure of 13.5 mm Hg at 298 K. The compound was also found to be nonvolatile and a nonelectrolyte. What is the molar mass of this compound? The nonvolatile, nonelectrolyte aspirin, C9H8O4 (180.1 g/mol), is soluble in chloroform CHCl3. Calculate the osmotic pressure (in atm) generated when 14.4 grams of aspirin are dissolved in 185 mL of a chloroform...
A team of students opened a soda pop can underwater and collected the gas released from...
A team of students opened a soda pop can underwater and collected the gas released from the head space in a 200 ml graduated cylinder. The students were careful to level the water in the cylinder with the water in the sink. Assume that the water and room temperature are the same at 22.0 degrees C. Here is their data: Volume of gas in the cylinder was 115.3 ml. At the temperature of the water, the vapor pressure of the...
A 300–mL volume of hydrogen is collected over water at 22 °C under a barometric pressure...
A 300–mL volume of hydrogen is collected over water at 22 °C under a barometric pressure of 740 mmHg. What is the volume of this hydrogen, at the same temperature and barometric pressure, when dry? (vapor pressure of water at 22 °C = 20 mmHg) the answer is 292 mL. PLEASE EXPLAIN HOW YOU GET THIS ANSWER :(
A sample of nitrogen gas is produced in a reaction and collected under water in a...
A sample of nitrogen gas is produced in a reaction and collected under water in a graduated cyliner. The temperature is 26.3 oC and the volume of gas is 45.6 mL. During this experiment the total pressure in the graduated cylinder is 745 mm Hg. How many grams of nitrogen were collected? (The vapor pressure of water at 26oC is 25.2 torr.)
1. A 34.32 mL sample of O2 gas was collected over water at 24 oC from the decomposition...
1. A 34.32 mL sample of O2 gas was collected over water at 24 oC from the decomposition of hydrogen peroxide. The barometric pressure in the room that day was 746.32 torr. A. Calculate the pressure of O2 gas in the system. B. Calculate the moles of gas collected. C. Calculate the moles of H2O2 initially present in the sample.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT