1. Combustion analysis of a 20.00 g sample of compound A, which contains C, H, N, and O atoms only, yields 47.41 g CO₂ (MW 44.01 g/mol), 10.59 g H₂O (MW 18.016 g/mol), and 9.011 g NO ₂ (MW 46.01 g/mol). What is the empirical formula of compound A? *Use the following atomic weights (in amu), H: 1.008; C: 12.01; №: 14.01; and O: 16.00.
1. Combustion analysis of a 20.00 g sample of compound A, which contains C, H, N, and O atoms only, yields 47.41 g CO₂ (MW 44.01 g/mol), 10.59 g H₂O (MW 18.016 g/mol), and 9.011 g NO ₂ (MW 46.01 g/mol). What is the empirical formula of compound A? *Use the following atomic weights (in amu), H: 1.008; C: 12.01; №: 14.01; and O: 16.00.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter2: Chemical Compounds
Section: Chapter Questions
Problem 123QRT
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Transcribed Image Text:1. Combustion analysis of a 20.00 g sample of compound A, which contains C, H, N, and O
atoms only, yields 47.41 g CO₂ (MW 44.01 g/mol), 10.59 g H₂O (MW 18.016 g/mol), and
9.011 g NO₂ (MW 46.01 g/mol). What is the empirical formula of compound A?
*Use the following atomic weights (in amu), H: 1.008; C: 12.01; N: 14.01; and O: 16.00.
2. Compound A has a molar mass of 204.226 g/mol. What is the molecular formula of
compound A?
3.
How many C atoms are present in 10.0 g of compound A?
4. What is the percent by mass composition of N in compound A?
5. Balance the combustion reaction for compound A.
_A+_0₂ → CO₂ +
H₂O + NO₂
6. Consider the combustion of 500.0 g of compound A with 800.0 g of O₂.
A. How much CO₂ (in grams) is produced in the reaction?
B. What are the masses of each reactant after the reaction?
C. If the percent yield for the reaction is 88.7%, what is the actual yield of NO₂?
7. What mass (in grams) of compound A is needed to prepare 750.0 mL of a 2.20 M solution?
8. What volume of a 2.20 M solution of compound A is needed to prepare 500.0 mL of a 0.5
M solution via dilution?
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