Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Determine how many molecules of H2CO are present in 33.0 mL of a 4.500 M solution of H2CO in water

Determine how many molecules of H2CO are present in 33.0 mL of a 4.500 M solution of H2CO in water

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

please help and kindly explain this to me

**Question:** Determine how many molecules of H₂CO are present in 33.0 mL of a 4.500 M solution of H₂CO in water. **Solution:** To solve this problem, we will use the following steps: 1. **Calculate the number of moles of H₂CO in the solution.** - **Molarity (M)** is defined as moles of solute per liter of solution. Therefore, to find the number of moles, we use the formula: \[ \text{Moles of H}_2\text{CO} = \text{Molarity} \times \text{Volume (L)} \] - Given the molarity is 4.500 M and the volume is 33.0 mL, convert the volume to liters: \[ 33.0 \, \text{mL} \times \frac{1 \, \text{L}}{1000 \, \text{mL}} = 0.0330 \, \text{L} \] - Calculate the moles: \[ \text{Moles of H}_2\text{CO} = 4.500 \, \text{mol/L} \times 0.0330 \, \text{L} = 0.1485 \, \text{mol} \] 2. **Calculate the number of molecules of H₂CO.** - Use Avogadro's number: \(6.022 \times 10^{23}\) molecules/mol. - Multiply the moles of H₂CO by Avogadro's number to find the number of molecules: \[ 0.1485 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol} = 8.945 \times 10^{22} \, \text{molecules} \] **Conclusion:** There are approximately \(8.945 \times 10^{22}\) molecules of H₂CO in 33.0 mL of the solution.
Transcribed Image Text:**Question:** Determine how many molecules of H₂CO are present in 33.0 mL of a 4.500 M solution of H₂CO in water. **Solution:** To solve this problem, we will use the following steps: 1. **Calculate the number of moles of H₂CO in the solution.** - **Molarity (M)** is defined as moles of solute per liter of solution. Therefore, to find the number of moles, we use the formula: \[ \text{Moles of H}_2\text{CO} = \text{Molarity} \times \text{Volume (L)} \] - Given the molarity is 4.500 M and the volume is 33.0 mL, convert the volume to liters: \[ 33.0 \, \text{mL} \times \frac{1 \, \text{L}}{1000 \, \text{mL}} = 0.0330 \, \text{L} \] - Calculate the moles: \[ \text{Moles of H}_2\text{CO} = 4.500 \, \text{mol/L} \times 0.0330 \, \text{L} = 0.1485 \, \text{mol} \] 2. **Calculate the number of molecules of H₂CO.** - Use Avogadro's number: \(6.022 \times 10^{23}\) molecules/mol. - Multiply the moles of H₂CO by Avogadro's number to find the number of molecules: \[ 0.1485 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol} = 8.945 \times 10^{22} \, \text{molecules} \] **Conclusion:** There are approximately \(8.945 \times 10^{22}\) molecules of H₂CO in 33.0 mL of the solution.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Concentration Terms
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
  • SEE MORE 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