### Ideal Gas Law Problem: Determining Moles of Chlorine Gas#### Problem Statement:Calculate the number of moles of chlorine gas at a temperature of 120.0°C and a pressure of 26.1 bar, occupying a vessel with a volume of 31.0 L. Use the ideal gas constant \( R = 0.08314 \, \text{L} \cdot \text{bar/mol} \cdot \text{K} \).#### Input Section:Enter the calculated number of moles (mol) using the on-screen keypad. The keypad includes numbers 0-9, a decimal point, and options to multiply by 10 (\( x10 \)) or clear the entry.### Explanation:This task involves using the ideal gas law equation:\[ PV = nRT \]Where:- \( P \) = Pressure (26.1 bar)- \( V \) = Volume (31.0 L)- \( n \) = Number of moles- \( R \) = Ideal gas constant (\( 0.08314 \, \text{L} \cdot \text{bar/mol} \cdot \text{K} \))- \( T \) = Temperature (in Kelvin; convert from Celsius by adding 273.15)The equation rearranges to solve for moles (\( n \)) as follows:\[ n = \frac{PV}{RT} \]#### Steps:1. **Convert Temperature**: \[ T = 120.0^\circ\text{C} + 273.15 = 393.15 \, \text{K} \]2. **Substitute Values**: \[ n = \frac{26.1 \times 31.0}{0.08314 \times 393.15} \]3. **Calculate the Result**: - Perform the multiplication and division to find \( n \).Use the keypad interface to input your calculated value and verify your result.

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Answered: How many moles of chlorine gas at…

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How many moles of chlorine gas at 120.0°C and 26.1 bar would occupy a vessel of 31.0 L? R = 0.08314 L· bar/mol·K.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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