Answer:
50.4 % of the water will be vapor
Explanation:
<u>Step 1:</u> Data given
Mass of water = 1.68 grams
volume of the flask = 5.3 L
Temperature = 65°C
Vapor pressure of water at 65°C = 187.5 mmHg = 0.2467 atm
<u>Step 2:</u> Calculate moles of H2O
p*V=n*R*T
⇒ p = the pressure of water = 0.2467 atm
⇒ V = the volume of the flask = 5.3 L
⇒ n = moles of water
⇒ R = gas constant = 0.08206 L*atm/ K*mol
⇒ T = the temperature = 65°C = 338 Kelvin
n = (p*V)/(R*T)
n = (0.2467 * 5.3) /(0.08206* 338)
n = 0.047 moles
<u>Step 3:</u> Calculate mass of water
Mass of water = moles of water * molar mass of water
Mass of water = 0.047 moles *18.02 g/mol
Mass of water = 0.84694 grams
<u>Step 4:</u> Calculate the percent of water vaporized
% = (0.84694 grams/1.68 grams) *100%
% = 50.4%
50.4 % of the water will be vapor
