Question

In: Chemistry

Mass of flask and foil(g) - 64.5297g Mass of flask, foil and condensed vapor - 64.9787g...

Mass of flask and foil(g) - 64.5297g

Mass of flask, foil and condensed vapor - 64.9787g

Temperature of boiling water bath - 101.2 C

Volume of flask (mL) - 153.0

Barometric pressure - 762.4 mmHg

Room temp - 23 C

Vapor pressure at room temperature - 100 mmHg

Calculate:
1. Uncorrected mass of condensed vapor(g)

2. Corrected density of air(g/L)

3. Average volume of flask (L)

4. Initial mass of air in flask (g)

5. Final partial pressure of air in flask (mmHg)

6.FInal mass of air in flask (g)

7.Mass of air lost (g)
8. Corrected mass of condensed vapor(g)
9. Molecuular weight (g/mol)

Expert Solution

queen_honey_blossom answered 1 year ago

Mass of Flask and foil (G)= 52.2997 Mass of Flask, foil, and condensed vapor(g) = 52.7528...

Mass of Flask and foil (G)= 52.2997 Mass of Flask, foil, and condensed vapor(g) = 52.7528 Temp of boiling water bath= 99.8 degrees C Volume of flask =140.1(ml) Barometric pressure (mmhg)= 762.2 Room temp= 23.1 C Vapor at room temp(mmHg) = 100.0 mmhm 1. What is uncorrected mass of condensed vapor (g)? 2. Corrected density of air(g/l) 3. Average volume of flask (g)? 4. Initial mass of air in flask(g)? 5. Final Partial Pressure of air in flask? 6. Final...

Mass of flask and foil (g) = 63.4842 Mass of flask, foil, and condesned vapor (g)...

Mass of flask and foil (g) = 63.4842 Mass of flask, foil, and condesned vapor (g) = 63.6995 Temperature of boiling water bath (C) = 95 degrees C Volume of flask (mL) = 134 Barometric pressre (mmHg) = 763.8 Room temperature (C) = 21.0 degrees C Vapor pressure at room temperature (mmHg) = 100 Find the following: 1) Uncorrected mass of condensed vapor (g) = ? 2). Corrected density of air (g/L) = ? 3). Average volume of flask (L)...

Mass of flask, stopper, and 5mL of water (g) 102.945 g Mass of flask, stopper, and...

Mass of flask, stopper, and 5mL of water (g) 102.945 g Mass of flask, stopper, and filled with water (g) 238.389 g Volume of gas space in flask (the difference between the above two measurements covnerted to mL) (L) .135444 L Mg(s) + HCl(aq) Reaction Trail 1 Trial 2 Mass of Mg(g) 0.008 0.007 Initial Pressure (atm) 0.9974 0.9945 Max Pressure (atm) 0.9980 0.007 Pressure Change (atm) 0.0006 0.0471 Temp (K) 295.7 296.1 a. Calculate the moles of H2 produced...

Mass of flask, stopper, and 5mL of water 102.945 g Mass of flask, stopper, and filled...

Mass of flask, stopper, and 5mL of water 102.945 g Mass of flask, stopper, and filled with water 238.389 g Volume of gas space in flask (the difference between the above two measurements converted to mL) (L) .135444 L NaHCO3 + HCl reaction Trial 1 Trial 2 Units Mass of NaHCO3 0.053 0.050 g Mass of system before reaction 117.026 117.189 g Mass of system after reaction 116.809 117.159 g Mass Change 0.217 0.030 g Initial Pressure 0.9876 0.9887 atm...

1. Determine the volume of the aluminum foil using the density of foil. Volume = mass...

1. Determine the volume of the aluminum foil using the density of foil. Volume = mass (g) x density g/cm3 Volume = 4.29 g/ 2.70 g/cm3 Volume= 1.59 cm3 2. Determine the volume of one atom of aluminum. 3. Determine the number of atoms of aluminum in the foil sample. 4. Determine the moles of aluminum. 5. Calculate Avogadro’s number.

Dumas Method Experiment: In this experiment, we measured a flask with an aluminum foil and elastic...

Dumas Method Experiment: In this experiment, we measured a flask with an aluminum foil and elastic band set up then added 4mL of methanol inside the flask and sealed with the foil covering and boiled in a water bath until all the liquid vaporized (this will drive out any air in the flask and push out all excess vapour). Then we cooled it to let the vapour condense and reweighed the flask with the vapour in it. The following questions...

A compound with molecular mass = 292.16 g/mol was dissolved in a 5.000 mL volumetric flask....

A compound with molecular mass = 292.16 g/mol was dissolved in a 5.000 mL volumetric flask. A 1.000 mL aliquot was withdrawn, placed in a 10.000 mL flask and diluted to volume. The apparent absorbance of the diluted solution at 340 nm was 0.827 in a 1.000 cm cuvette. To check for a possible stray light effect, this sample was diluted by exactly a factor of 2; the apparent absorbance was now 0.421. A reagent blank showed negligible absorbance. The...

A sample of water in the vapor phase (no liquid present) in a flask of constant...

A sample of water in the vapor phase (no liquid present) in a flask of constant volume exerts a pressure of 403 mmHg at 99°C. The flask is slowly cooled. i) Assuming no condensation, use the Ideal Gas Law to calculate the pressure of the vapor at 91°C; at 75°C. ii) Will condensation occur at 91°C? 75°C? iii) On the basis of your answers in i) and ii), predict the pressure exerted by the water vapor in the flask at...

Calculate the vapor pressure of a 20 % by mass sucrose (MW= 342.30 g/mol) solution. The...

Calculate the vapor pressure of a 20 % by mass sucrose (MW= 342.30 g/mol) solution. The vapor pressure of pure water is 23.8 torr. A) 23.50 torr B) 1.40 torr C) 23.8 torr D) 0.987 torr E) 4.44 torr

1.25-g of BaCl2 is placed in a 4.000 L volumetric flask. Then the volumetric flask is...

1.25-g of BaCl2 is placed in a 4.000 L volumetric flask. Then the volumetric flask is filled with D.I. water to the 4.000 L mark. All the BaCl2 goes into the solution. Assume the density of the solution is 1.00 g/mL. What is the mass/mass (m/m) % and the mass/volume (m/v) of the solution?