The number of moles in a 2.00-L volume of air at 37.0°C can be calculated using the ideal gas law formula PV = nRT, by utilizing the given temperature, a standard pressure of 1 atm, and known constants.
To calculate the number of moles in a 2.00-L volume of air at body temperature (37.0°C), we need to use the ideal gas law, which is PV = nRT. Here, P represents the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. Assuming that the pressure P is 1 atm (since the person is at or near sea level and not undergoing any unusual pressure conditions), and converting the given temperature to Kelvin (37.0°C equal to 310.15 K), we can rearrange the formula to solve for the number of moles (n).
The ideal gas constant (R) is 0.0821 (Latm)/(molK). Plugging the values into the ideal gas law equation, we get:
(1 atm) × (2.00 L) = n × (0.0821 Latm/molK) × (310.15 K)
To find n, we simply divide the product of P and V by the product of R and T:
n = ((1 atm) × (2.00 L)) / ((0.0821 Latm/molK) × (310.15 K))
After doing the calculation, we find out the number of moles in the 2.00-L volume of air at body temperature.
The complete question is- Calculate the number of moles in the 2.00-l volume of air in the lungs of the average person. note that the air is at 37.0 degree celcius (body temperature).