Question

ley de los gases ideales pv=terapia de reemplazo de n - tratamiento (trn)
constante del gas ideal r = 8.314 l kpa / (mol k) 0 r = 0.0821 l atm / (mol k)
presión atmosférica estándar 1 atm = 101.3 kpa
conversión de celsius a kelvin k = °c + 273.15
temperatura del aire es de 295 k, ¿cuántos moles de oxígeno hay en el pulmón?
a. 0.026 moles
b. 0.12 moles
do. 2.6 moles
d. 13 moles

Explanation:

Step1: Recall ideal - gas law

The ideal - gas law is $PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is the number of moles, $R$ is the ideal - gas constant, and $T$ is temperature. We assume standard atmospheric pressure $P = 1\ atm=101.3\ kPa$ and let's assume a typical lung volume $V = 3\ L$ (a reasonable estimate for a normal - sized lung at rest), $R = 0.0821\frac{L\cdot atm}{mol\cdot K}$, and $T = 295\ K$.
We need to solve for $n$, so we can re - arrange the ideal - gas law formula to $n=\frac{PV}{RT}$.

Step2: Substitute values

Substitute $P = 1\ atm$, $V = 3\ L$, $R = 0.0821\frac{L\cdot atm}{mol\cdot K}$, and $T = 295\ K$ into the formula $n=\frac{PV}{RT}$.
$n=\frac{1\ atm\times3\ L}{0.0821\frac{L\cdot atm}{mol\cdot K}\times295\ K}$
$n=\frac{3}{0.0821\times295}$
$n=\frac{3}{24.2195}\approx0.12\ mol$

Answer:

B. 0.12 moles