Homework Answers
sample 1
vapor pressure of water at the given temperature = 18.7 mmHg
vapor pressure of dry hydrogen = total pressure - water vapor pressure.
= 747.776 mmHg - 18.7 mmHg
= 729.976 mmHg
temperature = 20.8 + 273 k
= 293.8K
R = 0.0821lit.atm/k.mol
volume of gas = 22.65 ml
= 0.02265 lit
number of moles of hydrogen = pV/RT
= 729.976 mmHg x 0.02265 lit / 0.0821lit.atm/k.mol x 293.8K
= 0.6846 moles
mass of magnesium ribbon
1 equivalent of magnesium metal = 1 equivalent of hydrogen gas
so numbe rof moles of Mg = moles of hydrogen
= 0.6846 moles
mass of Mg ribbon = 0.6846 moles x 24 g/mol
= 16.43 g
sample2 ----- same Temperature
vapor pressure of water at the given temperature = 18.7 mmHg
vapor pressure of dry hydrogen = total pressure - water vapor pressure.
= 747.776 mmHg - 18.7 mmHg
= 729.976 mmHg
temperature = 20.8 + 273 k
= 293.8K
R = 0.0821lit.atm/k.mol
volume of gas = 22.12 ml
= 0.02212 lit
number of moles of hydrogen = pV/RT
= 729.976 mmHg x 0.02212 lit / 0.0821lit.atm/k.mol x 293.8K
= 0.6694 moles of hydrogen gas = moles of Mg
mass of Mg ribbon = moles of Mg ribbon metal x 24 g/mol
= 0.6694 x 24 g/mol
= 16.0656 g
average mass of Mg ribbon = (16.43 g + 16.0656 g )/2
= 16.2478 g
----------------------------------------------------------------------
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Data Sheet Unknown Number Sample 2 Sample 1 Volume of Ha gas (ml.) 22.65 22.12 Temperature...
Date: 7 Record the barometric pressure. 8. Repeat this experiment with the second piece of magnesium...
Date: 7 Record the barometric pressure. 8. Repeat this experiment with the second piece of magnesium ribbon. 9. Untwist the wire from the piece of fiberglass. Rinse the wire, fiberglass square, and stopper, place them in the container, and return the container to the instructor's desk. The table of temperature/Vapor pressure of water is in your textbook and in the back of your laboratory manual. The density of mercury is 13.6 g/mL. 61302083 Data Sheet Unknown Number Sample 2 40.8m2...
The vapor pressure of water changes with temperature, as shown here. T(∘C) P(torr) 21 18.7 22...
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Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip...
Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip of magnesium metal with 4.00 mL of 4.0 M hydrochloric acid and collected the hydrogen gas produced using the experimental setup you see at the station. Unfortunately, the student forgot to record the mass of the metal before they reacted it with acid. Determine the mass of the magnesium metal the student used in the experiment. For this experiment assume the pressure of the...
Temperature °C Water Vapor Pressure (mmHg) Magnesium metal is reacted with hydrochloric acid to produce hydrogen...
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The vapor pressure of water changes with temperature, as shown here. T(∘C) P(torr) 21 18.7 22...
The vapor pressure of water changes with temperature, as shown here. T(∘C) P(torr) 21 18.7 22 19.8 23 21.1 24 22.4 25 23.8 26 25.2 27 26.7 28 28.4 29 30.0 30 31.8 The values above go in this order 21 is T(C) and 18.7 is (Ptorr) goes in this order all the way down A student designs an ammeter (a device that measures electrical current) that is based on the electrolysis of water into hydrogen and oxygen gases. When...
Date Post-Lab Questions If your partner did not take into account the vapor pressure of water whe...
Date Post-Lab Questions If your partner did not take into account the vapor pressure of water when calculating the moles of hydrogen produced, would the mass of Mg that was calculated at the end of the experiment be too high or too low? nced haf t ribbon are coated with white MgO, would this cause the mass of Mg that you calculate to be too high or too low? Why? 3. Instead of a strip of pure Mg nibbon, you...
Equal molar amounts of neon were collected over water in two identical 6.0-L flasks, one being...
Equal molar amounts of neon were collected over water in two
identical 6.0-L flasks, one being at 30 degrees Celcius and the
other being at 20 degrees Celcius, respectively. The difference of
respective total pressures in two flasks was 845.8 torr. Use the
provided table of vapor pressure versus temperature (picture) to
calculate the number of moles of neon collected in each flask.
uuulements Vapor Pressure of Water at Selected Temperatures (*) Temperature, T°C Vapor pressure, I Pvapor Torr I...
A handbook lists the normal haline pint of an organic liquid is enthalpy of vaporization as...
A handbook lists the normal haline pint of an organic liquid is enthalpy of vaporization as 59.8 kJ/mol. Calculate the vapor pressure in tort of this compound at 138.0°C 4. Hydrazine, N2H4, has a normal boiling point of 113.5°C and a critical point at 380.0°C and 145.4 atm. Estimate the vapor pressure of hydrazine at 40.0°C. (Treat the critical point as last point on the vapor pressure curve.) Clausius CS Vapor Pressure of Water at Different Temperatures Temperature (C) Vapor...
83 Name: Gas Laws Lab Prelab questions: Your instructor may ask you to answer these in...
83 Name: Gas Laws Lab Prelab questions: Your instructor may ask you to answer these in your lab notebook in a online or they may ask you to write your answers in your lab manual and submit them before starting your experiment. Follow your instructor's directions. "prelab" section, 1. What is an ideal gas? 2. Using Appendix B from your textbook complete the following table: (remember 760 mm Hg = 1 atm) Temperature (°C) 18 19 Pressure (mm Hg) Pressure...
83 Name: Gas Laws Lab Prelab questions: Your instructor may ask you to answer these in...
83 Name: Gas Laws Lab Prelab questions: Your instructor may ask you to answer these in your lab notebook in a online or they may ask you to write your answers in your lab manual and submit them before starting your experiment. Follow your instructor's directions. "prelab" section, 1. What is an ideal gas? 2. Using Appendix B from your textbook complete the following table: (remember 760 mm Hg = 1 atm) Temperature (°C) 18 19 Pressure (mm Hg) Pressure...
Date: 7 Record the barometric pressure. 8. Repeat this experiment with the second piece of magnesium ribbon. 9. Untwist the wire from the piece of fiberglass. Rinse the wire, fiberglass square, and stopper, place them in the container, and return the container to the instructor's desk. The table of temperature/Vapor pressure of water is in your textbook and in the back of your laboratory manual. The density of mercury is 13.6 g/mL. 61302083 Data Sheet Unknown Number Sample 2 40.8m2...
Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip of magnesium metal with 4.00 mL of 4.0 M hydrochloric acid and collected the hydrogen gas produced using the experimental setup you see at the station. Unfortunately, the student forgot to record the mass of the metal before they reacted it with acid. Determine the mass of the magnesium metal the student used in the experiment. For this experiment assume the pressure of the...
Temperature °C Water Vapor Pressure (mmHg) Magnesium metal is reacted with hydrochloric acid to produce hydrogen gas. A sample of hydrogen gas is collected over water in a eudiometer. Calculate the mass (in grams) of magnesium metal needed to produce 39.0 mL of hydrogen gas at an atmospheric pressure of 739 mmHg and a temperature of 25.9 °C. 20 17.5 22 19.8 24 22.4 Mass of Mg - g 26 25.2 28 28.3 30 31.8
Date Post-Lab Questions If your partner did not take into account the vapor pressure of water when calculating the moles of hydrogen produced, would the mass of Mg that was calculated at the end of the experiment be too high or too low? nced haf t ribbon are coated with white MgO, would this cause the mass of Mg that you calculate to be too high or too low? Why? 3. Instead of a strip of pure Mg nibbon, you...
Equal molar amounts of neon were collected over water in two
identical 6.0-L flasks, one being at 30 degrees Celcius and the
other being at 20 degrees Celcius, respectively. The difference of
respective total pressures in two flasks was 845.8 torr. Use the
provided table of vapor pressure versus temperature (picture) to
calculate the number of moles of neon collected in each flask.
uuulements Vapor Pressure of Water at Selected Temperatures (*) Temperature, T°C Vapor pressure, I Pvapor Torr I...
A handbook lists the normal haline pint of an organic liquid is enthalpy of vaporization as 59.8 kJ/mol. Calculate the vapor pressure in tort of this compound at 138.0°C 4. Hydrazine, N2H4, has a normal boiling point of 113.5°C and a critical point at 380.0°C and 145.4 atm. Estimate the vapor pressure of hydrazine at 40.0°C. (Treat the critical point as last point on the vapor pressure curve.) Clausius CS Vapor Pressure of Water at Different Temperatures Temperature (C) Vapor...
83 Name: Gas Laws Lab Prelab questions: Your instructor may ask you to answer these in your lab notebook in a online or they may ask you to write your answers in your lab manual and submit them before starting your experiment. Follow your instructor's directions. "prelab" section, 1. What is an ideal gas? 2. Using Appendix B from your textbook complete the following table: (remember 760 mm Hg = 1 atm) Temperature (°C) 18 19 Pressure (mm Hg) Pressure...
83 Name: Gas Laws Lab Prelab questions: Your instructor may ask you to answer these in your lab notebook in a online or they may ask you to write your answers in your lab manual and submit them before starting your experiment. Follow your instructor's directions. "prelab" section, 1. What is an ideal gas? 2. Using Appendix B from your textbook complete the following table: (remember 760 mm Hg = 1 atm) Temperature (°C) 18 19 Pressure (mm Hg) Pressure...
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