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Answer to Question #66124 in General Chemistry for Samuel
Question #66124
Data: Room Temperature: 72 F
Mass of magnesium ribbon: 0.044g
Atmospheric pressure in room: .985 atm
Temp of water in beaker: 23 C
Volume of gas in the tube: 43.60g
1. Use the mass of the magnesium ribbon to find the moles of gas produced using stoichiometry.
2. Change the volume of gas collected to liters.
3. Find the temperature of the gas you collected in kelvin.
4. Convert the atmospheric pressure to atm.
5. Use the number of moles, the volume, temp, and pressure of the gas that you found above to solve for the experimental gas constant R using the ideal gas law.
Thank you so much for the help!
Mass of magnesium ribbon: 0.044g
Atmospheric pressure in room: .985 atm
Temp of water in beaker: 23 C
Volume of gas in the tube: 43.60g
1. Use the mass of the magnesium ribbon to find the moles of gas produced using stoichiometry.
2. Change the volume of gas collected to liters.
3. Find the temperature of the gas you collected in kelvin.
4. Convert the atmospheric pressure to atm.
5. Use the number of moles, the volume, temp, and pressure of the gas that you found above to solve for the experimental gas constant R using the ideal gas law.
Thank you so much for the help!
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