Homework Help is Here – Start Your Trial Now!
Science
Chemistry
How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 40.0 L?

How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 40.0 L?

Chemistry
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...
See similar textbooks
icon
Related questions
Question

I got this answer wrong and I want to know how 

**Problem:** *Question 7 of 14* How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 40.0 L? **Answer:** 0.807 mol **Explanation:** This is a chemistry problem requiring the use of the ideal gas law equation: \[ PV = nRT \] Where: - \( P \) = pressure in atmospheres (atm) - \( V \) = volume in liters (L) - \( n \) = number of moles - \( R \) = ideal gas constant (0.0821 L·atm/mol·K) - \( T \) = temperature in Kelvin (K) **Calculation Steps:** 1. Convert the temperature from Celsius to Kelvin: \[ T(K) = 120 + 273.15 = 393.15 \, K \] 2. Rearrange the ideal gas law to solve for the number of moles (\( n \)): \[ n = \frac{PV}{RT} \] 3. Insert the known values into the equation: \[ n = \frac{(33.3 \, \text{atm})(40.0 \, \text{L})}{(0.0821 \, \text{L·atm/mol·K})(393.15 \, \text{K})} \] 4. Calculate the number of moles: \[ n \approx 0.807 \, \text{mol} \] This calculation gives the number of moles of chlorine gas under the specified conditions.
Transcribed Image Text:**Problem:** *Question 7 of 14* How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 40.0 L? **Answer:** 0.807 mol **Explanation:** This is a chemistry problem requiring the use of the ideal gas law equation: \[ PV = nRT \] Where: - \( P \) = pressure in atmospheres (atm) - \( V \) = volume in liters (L) - \( n \) = number of moles - \( R \) = ideal gas constant (0.0821 L·atm/mol·K) - \( T \) = temperature in Kelvin (K) **Calculation Steps:** 1. Convert the temperature from Celsius to Kelvin: \[ T(K) = 120 + 273.15 = 393.15 \, K \] 2. Rearrange the ideal gas law to solve for the number of moles (\( n \)): \[ n = \frac{PV}{RT} \] 3. Insert the known values into the equation: \[ n = \frac{(33.3 \, \text{atm})(40.0 \, \text{L})}{(0.0821 \, \text{L·atm/mol·K})(393.15 \, \text{K})} \] 4. Calculate the number of moles: \[ n \approx 0.807 \, \text{mol} \] This calculation gives the number of moles of chlorine gas under the specified conditions.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Mole Concept
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS