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The solubility of N₂ in blood is a serious problem for divers breathing compressed air (78% N₂ by volume) at depths greater than 50 ft.(c) Find the volume (in mL) of N₂, measured at 25°C and 1.00 atm, released per liter of blood when a diver at a depth of 50. ft rises to the surface ( kH for N₂ in water at 25°C is 7.0x10⁻⁴ mol/L . atm and at 37°C is 6.2x10⁻⁴ mol/L . atm; assume d of water is 1.00 g/mL).

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anvitanvar032

c)  Volume = 19.7 mL Step 1: Given data Pressure at sea level = 1.00 ATM Pressure at 50 ft = 2.47535 atm kH for N2 in water at 25°C is 7.0 × 10−4 mol/L· atm Molarity (M) = kH x P Step 2: Calculate molarity M at sea level:

M = 7.0*10^-4 * (1.00atm * 0.78) =

5.46*10^-4 mol/LM at 50ft:M

= 7.0*10^-4 * (2.47535atm * 0.78)

= 13.5*10^-4 mol/LWe have to find the volume of N2.

To find the volume we have to find the number of moles present. This can be calculated by finding the difference between M at 50 ft and M at sea level.

n = 13.5*10^-4 mol/L - 5.46*10^-4 mol/L n

= 8.04*10^-4 mol/LStep

3: Calculate volume P*V=nRT with P = 1.00 atm with

V = unknown with n =  8.04*10^-4 mol/L  *1L = 8.04*10^-4with

R= 0.0821 atm * L/ mol *K with

T = 25 °C = 273+25 = 298 K°As Volume is unknown, we will arrange the formula as needed:

V = nRT ÷ P   = 8.04*10^-4 mol/L × 0.0821 atm * L/ mol *K × 298 K° ÷ 1.00 atm   =  0.0197L   = 19.7 mL. Thus, the volume is 19.7 mL.

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