Homework Help (chemistry)
By xntejano
@xntejano (1)
United States
April 30, 2007 10:41pm CST
The partial pressure of CO2 in contact with human arterial blood is 46 torr. The Henry's law constant for CO2 in blood plasma at 37 Celcius is .51ml Co2/ml plasma at 1 atm of CO2. Calculate the amount of carbon dioxide in milliliters, dissolved in a milliliter of arterial blood.
4 responses
@icedtee (31)
• Canada
17 May 07
Henry's law states p = kc
where p is partial pressure, k is henry's constant and c = concentration.
Step 1: 46torr = 0.51mLCO2/mLplasma * c
Step 2: Convert to equal units: 46 torr = 0.06atm
Step 3: Solve: (0.06atm / 0.51(mLCO2/mL plasma))= c
Assuming 1mL of plasma,
c = 0.118mL
@dianagnes (1088)
• Singapore
15 May 07
Its cool you posting what that you dont know and seek for help here.Sorry,i dont know and i cant help.Im not good at chemistry and i am also trying my very best to improve it!
@cursedsoul (925)
• India
15 May 07
I think I've done something similar. Which year are you in and how do you convert torr to its SI unit eqivalent?
