This preview shows page 1. Sign up to view the full content.
Unformatted text preview: for the pressure of the hydrogen gas, H 2 . Rearrange the formula to solve for P. (Show work, use units and dimensional analysis. All units should cancel except the unit for pressure. Remember significant figures.) [(.0016)*(.08205)((liter*atm)/(mol*K))(296K)]/.04162 liters= .93atm 4. This calculated pressure is in the units of atmospheres. Convert this pressure to mm Hg. (1 atm = 760 mm Hg) Show your work clearly and completely. (.93atm*760mm Hg)/1atm= 706.8 mm Hg 5. Using the vapor pressure of water at room temperature (Table I) and your calculated hydrogen gas pressure, compute the total atmospheric pressure. Remember, in order to add two values together, the units for both numbers need to be the same. Show your work and units! (727.9mm Hg*1atm)/760mm Hg Final atmospheric pressure .96atm (Units??)...
View
Full
Document
This note was uploaded on 04/18/2008 for the course CHEM 1151L taught by Professor Stone during the Spring '08 term at Clayton.
 Spring '08
 STONE
 pH

Click to edit the document details