The volume of the pressure vessel is 0.44 liters. The number of moles of H2 gas formed can be determined for the unknown samples. Enter the corrected gas pressures (after subtracting the water vapor pressure) for unknowns 1 and 2. For Unknowns 1 & 2, Make sure you subtract 20 from the pressure in torr measured in the lab to obtain the corrected pressure. Unknown 1 - ? torr Unknown 2 - ? torr For the next two unknowns, use the ideal gas equation, and the volume obtained above to calculate the number of moles of H2 gas produced during each unknown run. Assume the gas temperature at the end of each run is 22 deg c Unknown 1 - ? moles H2 Unknown 2 - moles H2 Use the formula PV=nRT to solve for n (number of moles). You know the volume, or "V" (0.44 L), you know the value of R (0.0821 L x atm/mol x K). Make sure you convert the temperature to Kelvin and the pressure to atm before plugging into this formula.
The volume of the pressure vessel is 0.44 liters. The number of moles of H2 gas formed can be determined for the unknown samples. Enter the corrected gas pressures (after subtracting the water vapor pressure) for unknowns 1 and 2. For Unknowns 1 & 2, Make sure you subtract 20 from the pressure in torr measured in the lab to obtain the corrected pressure. Unknown 1 - ? torr Unknown 2 - ? torr For the next two unknowns, use the ideal gas equation, and the volume obtained above to calculate the number of moles of H2 gas produced during each unknown run. Assume the gas temperature at the end of each run is 22 deg c Unknown 1 - ? moles H2 Unknown 2 - moles H2 Use the formula PV=nRT to solve for n (number of moles). You know the volume, or "V" (0.44 L), you know the value of R (0.0821 L x atm/mol x K). Make sure you convert the temperature to Kelvin and the pressure to atm before plugging into this formula.
Related textbook solutions
Basic Chemistry
Principles of Chemistry Molecular Approach
Principles of Chemistry Molecular Approach
Chemistry: Structure and Properties
Chemistry: A Molecular Approach
Chemistry: A Molecular Approach
Principles of Chemistry: A Molecular Approach
