a mix of gases is collected over water at 14C (287.15Kelvin) and has a total pressure of .981 atm and occupies 55mL. How many grams of water escaped into the vapor state? Hint: What is the vapor Pressure of water?
This has gotten me completely confused.
n=PV/RT
n=(.981*.055)/(.08206*287.15)
This makes the molarity .0022897674
Since Molarity = Mol/G divide .0022897674 by 16 and you get 1.431104611
I know this isn't the answer. Where did i go wrong and why do i need the vapor pressure of water?
Which btw is 12 mmHg, which is inevitably .0157894737 atm
HELP! I'm going crazy over this question!
