**Question 13: Calculating Moles of Air in the Lungs****Problem Statement:**Your lungs hold 4.2 L of air at a temperature of 27°C and a pressure of 101.3 kPa. How many moles of air do your lungs hold? (R = 8.31 J/mol·K)**Options:**A) 0.19 moles B) 0.15 moles C) 0.23 moles D) 0.17 moles E) 0.21 moles ### Explanation:To solve this problem, we use the Ideal Gas Law equation:\[ PV = nRT \]where:- $ P $ = pressure (in kPa)- $ V $ = volume (in liters)- $ n $ = number of moles (what we need to find)- $ R $ = ideal gas constant (8.31 J/mol·K)- $ T $ = temperature (in Kelvin, K)**Step-by-Step Solution:**1. **Convert Temperature to Kelvin:** \[ T(K) = 27°C + 273 = 300K \]2. **Rearrange the Ideal Gas Law Equation to Solve for $ n $:** \[ n = \frac{PV}{RT} \]3. **Plug the Given Values into the Equation:** \[ P = 101.3 kPa \] \[ V = 4.2 L \] \[ T = 300 K \] \[ R = 8.31 J/mol·K \]4. **Calculate using the Ideal Gas Law:** \[ n = \frac{(101.3 \, \text{kPa}) (4.2 \, \text{L})}{(8.31 \, \frac{J}{\text{mol} \cdot K})(300 \, \text{K})} \] To ensure the units are consistent for R, we may need to convert kPa to Pa (1 kPa = 1000 Pa): \[ n = \frac{(101300 \, \text{Pa}) (4.2 \, \text{L})}{(8.31 \, \frac{J}{\text{mol}

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13) Your lungs hold 4.2 L of air at a temperature of 27°C and a pressure of 101.3 kPa. How many moles of air do your lungs hold? (R = 8.31 J/mol. K) A) 0.19 moles B) 0.15 moles C) 0.23 moles D) 0.17 moles E) 0.21 moles

13) Your lungs hold 4.2 L of air at a temperature of 27°C and a pressure of 101.3 kPa. How many moles of air do your lungs hold? (R = 8.31 J/mol. K) A) 0.19 moles B) 0.15 moles C) 0.23 moles D) 0.17 moles E) 0.21 moles

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

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