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11111nata11111 [884]
3 years ago
14

Consider 1.5 L of air in a patents lungs at 37.0 C and 1.00 atm pressure. What is the volume would this air occupy if it were at

25 C under a pressure of 5.00 x 10^2 atm?
Chemistry
1 answer:
SSSSS [86.1K]3 years ago
5 0

Answer:

0.00288 L = 2.88 mL.

Explanation:

  • To calculate the no. of moles of a gas, we can use the general law of ideal gas: <em>PV = nRT.</em>

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R is the general gas constant.

T is the temperature of the gas in K.

  • If n is constant, and have two different values of (P, V and T):

<em>P₁V₁T₂ = P₂V₂T₁</em>

<em></em>

P₁ = 1.0 atm, V₁ = 1.5 L, T₁ = 37°C + 273 = 310 K.

P₂ = 500.0 atm, V₂ = ??? L, T₂ = 25°C + 273 = 298 K.

<em>∴ V₂ = P₁V₁T₂/P₂T₁</em> = (1.0 atm)(1.5 L)(298 K)/(500.0 atm)(310 L) = <em>0.00288 L = 2.88 mL.</em>

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