Homework Help is Here – Start Your Trial Now!
Science
Chemistry
If you have 155 mL solution of a 0.762 M FeCb solution, how many g FeCb are contained in this sample? 155 ml solution motFect x 0.762 STARTING AMOUNT molFeC. 155 ml solution 0.762 mol FeCh x- 1 mol FeCl ADD FACTOR DELETE ANSWER RESET *( ) 1000 0.1 124 4.92 1.92 0.203 162.2 55.85 12.6 35.45 100 25.1 7.28 x 10 6.60 1 0.762 155 0.118 19.2 0.01 mol FeCt g FeCl/mol FeCl L solution g FeCh g CF M FeCb g Fe* ml solution mol FeCl:/L solution

If you have 155 mL solution of a 0.762 M FeCb solution, how many g FeCb are contained in this sample? 155 ml solution motFect x 0.762 STARTING AMOUNT molFeC. 155 ml solution 0.762 mol FeCh x- 1 mol FeCl ADD FACTOR DELETE ANSWER RESET *( ) 1000 0.1 124 4.92 1.92 0.203 162.2 55.85 12.6 35.45 100 25.1 7.28 x 10 6.60 1 0.762 155 0.118 19.2 0.01 mol FeCt g FeCl/mol FeCl L solution g FeCh g CF M FeCb g Fe* ml solution mol FeCl:/L solution

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
100%

How do I fill this out?

 

# Calculating Mass of FeCl₃ in a Solution ## Question If you have a 155 mL solution of a 0.762 M FeCl₃ solution, how many grams of FeCl₃ are contained in this sample? ## Setup - **Starting Amount:** 0.762 mol/L FeCl₃ - **Volume of Solution:** 155 mL ## Calculation Steps 1. **Convert Volume to Liters:** - Given 155 mL solution. This is converted to liters as \( \frac{155}{1000} = 0.155 \) L. 2. **Determine the moles of FeCl₃:** - Use the molarity equation: - \( \text{Moles of FeCl₃} = \text{Molarity} \times \text{Volume in L} \) - \( \text{Moles of FeCl₃} = 0.762 \, \text{mol/L} \times 0.155 \, \text{L} = 0.11811 \, \text{mol} \) 3. **Convert moles to grams:** - **Molar Mass of FeCl₃:** (commonly calculated as 162.2 g/mol; confirm with specific work if precise). - **Formula:** \( \text{grams} = \text{moles} \times \text{molar mass} \) - **Calculation:** \( 0.11811 \, \text{mol} \times 162.2 \, \text{g/mol} = 19.15 \, \text{g} \) ## Tool Interface - **Control Buttons:** - **Add Factor:** Allows you to add multiplication or division factors. - **Delete:** Use to remove steps. - **Answer:** To display the final outcome. - **Reset:** Clears the current calculation to start fresh. - **Conversion Options:** - Available units for conversion (grams, moles, liters, etc.). - Specific constants and values provided for quick calculations, including molar masses.
Transcribed Image Text:# Calculating Mass of FeCl₃ in a Solution ## Question If you have a 155 mL solution of a 0.762 M FeCl₃ solution, how many grams of FeCl₃ are contained in this sample? ## Setup - **Starting Amount:** 0.762 mol/L FeCl₃ - **Volume of Solution:** 155 mL ## Calculation Steps 1. **Convert Volume to Liters:** - Given 155 mL solution. This is converted to liters as \( \frac{155}{1000} = 0.155 \) L. 2. **Determine the moles of FeCl₃:** - Use the molarity equation: - \( \text{Moles of FeCl₃} = \text{Molarity} \times \text{Volume in L} \) - \( \text{Moles of FeCl₃} = 0.762 \, \text{mol/L} \times 0.155 \, \text{L} = 0.11811 \, \text{mol} \) 3. **Convert moles to grams:** - **Molar Mass of FeCl₃:** (commonly calculated as 162.2 g/mol; confirm with specific work if precise). - **Formula:** \( \text{grams} = \text{moles} \times \text{molar mass} \) - **Calculation:** \( 0.11811 \, \text{mol} \times 162.2 \, \text{g/mol} = 19.15 \, \text{g} \) ## Tool Interface - **Control Buttons:** - **Add Factor:** Allows you to add multiplication or division factors. - **Delete:** Use to remove steps. - **Answer:** To display the final outcome. - **Reset:** Clears the current calculation to start fresh. - **Conversion Options:** - Available units for conversion (grams, moles, liters, etc.). - Specific constants and values provided for quick calculations, including molar masses.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
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