**Understanding the Calculation of Moles of Air in a Given Volume**When calculating the number of moles of air in a 2.0 L bottle at 19°C and 747 mm Hg, we use the Ideal Gas Law, which is represented by the formula:**PV = nRT****Where:**- **P** is the pressure of the gas.- **V** is the volume of the gas.- **n** is the number of moles of gas.- **R** is the ideal gas constant.- **T** is the temperature in Kelvin.**Given Values:**- Volume (V) = 2.0 liters- Temperature (T) = 19°C = 19 + 273 = 292 K (conversion from Celsius to Kelvin)- Pressure (P) = 747 mm Hg**Values for the Ideal Gas Constant (R):**1. **R = 0.0821 (L atm) / (mol K)**2. **R = 62.4 (L mm Hg) / (K mol)**3. **R = 8.31 (L kPa) / (K mol)**In this scenario, since the pressure is given in mm Hg, we'll use the second value for R:**R = 62.4 (L mm Hg) / (K mol)**Using these variables in the ideal gas law formula, we can solve for the number of moles (n) of air in the bottle.This educational example illustrates how to apply the Ideal Gas Law to find the quantity of moles in a given volume of gas under specific conditions of temperature and pressure.

Given that P = 747 mm Hg V = 2 litres T= 19°C= 273.15 + 19= 292.15 K n= number of moles. Now, PV=nRT Here we use R= 62.4 (L mm Hg)/(K mol) in order to match the units in which P, V and T are given. Therefore, PV = nRT or 747*2 = n*62.4*292.15 or n = 1494÷18230.16 or n = 0.0819 moles. Therefore at these given conditions, a 2 litre bottle will hold 0.0819 moles of air.

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How many moles of air are there in a 2.0 L bottle at 19°C and 747 mm Hg? • PV=nRT • R = 0.0821 (L atm) (mol K) • R = 62.4 (L mm Hg) (K mol) • R = 8.31 (L kPa) (K mol)

Human Anatomy & Physiology (11th Edition)

11th Edition

ISBN:9780134580999

Author:Elaine N. Marieb, Katja N. Hoehn

Publisher:Elaine N. Marieb, Katja N. Hoehn

Chapter1: The Human Body: An Orientation

Section: Chapter Questions

Problem 1RQ: The correct sequence of levels forming the structural hierarchy is A. (a) organ, organ system,...

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