Molar Masses A = 12.98 D = 13.43– X = 22.40–2 E = 19.26 Z = 4.032 mole mole G = 16.42 mole mole A compound, with molar mass 245.85 was analyzed and found to contain 16.39 % D, 23.50 % E, and 60.11 %G.Using the molar masses and molecular weight provided above please determine the empirical and molecular formulas of the compound. mole Empirical Formula = type your answer.. Molecular Formula = type your answer.
Molar Masses A = 12.98 D = 13.43– X = 22.40–2 E = 19.26 Z = 4.032 mole mole G = 16.42 mole mole A compound, with molar mass 245.85 was analyzed and found to contain 16.39 % D, 23.50 % E, and 60.11 %G.Using the molar masses and molecular weight provided above please determine the empirical and molecular formulas of the compound. mole Empirical Formula = type your answer.. Molecular Formula = type your answer.
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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### Molar Masses
#### Elemental Molar Masses:
- \( A = 12.98 \, \frac{g}{mole} \)
- \( G = 16.42 \, \frac{g}{mole} \)
- \( D = 13.43 \, \frac{g}{mole} \)
- \( X = 22.40 \, \frac{g}{mole} \)
- \( E = 19.26 \, \frac{g}{mole} \)
- \( Z = 4.032 \, \frac{g}{mole} \)
#### Compound Analysis
A compound with a molar mass of \( 245.85 \, \frac{g}{mole} \) was analyzed and found to contain:
- \( 16.39 \% \, D \)
- \( 23.50 \% \, E \)
- \( 60.11 \% \, G \)
Using the molar masses and molecular weight provided above, please determine the empirical and molecular formulas of the compound.
#### Input Fields:
##### Empirical Formula:
\[ \text{Empirical Formula} = \, \text{(type your answer...)} \]
##### Molecular Formula:
\[ \text{Molecular Formula} = \, \text{(type your answer...)} \]
---
Please enter your answers in the provided input fields.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F19b343d3-def3-436d-96c5-7f330515e000%2F11306384-70e7-4348-bdcd-421cfab5c458%2Fkhjvvr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:---
### Molar Masses
#### Elemental Molar Masses:
- \( A = 12.98 \, \frac{g}{mole} \)
- \( G = 16.42 \, \frac{g}{mole} \)
- \( D = 13.43 \, \frac{g}{mole} \)
- \( X = 22.40 \, \frac{g}{mole} \)
- \( E = 19.26 \, \frac{g}{mole} \)
- \( Z = 4.032 \, \frac{g}{mole} \)
#### Compound Analysis
A compound with a molar mass of \( 245.85 \, \frac{g}{mole} \) was analyzed and found to contain:
- \( 16.39 \% \, D \)
- \( 23.50 \% \, E \)
- \( 60.11 \% \, G \)
Using the molar masses and molecular weight provided above, please determine the empirical and molecular formulas of the compound.
#### Input Fields:
##### Empirical Formula:
\[ \text{Empirical Formula} = \, \text{(type your answer...)} \]
##### Molecular Formula:
\[ \text{Molecular Formula} = \, \text{(type your answer...)} \]
---
Please enter your answers in the provided input fields.
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