compound has the composition: carbon 37.21%; hydrogen 7.83%; and chlorine 54.96%. If its MW is 385 g/mol, determine (a) the empirical formula (b) the molecular formula. C H Cl Mass of element (in g) (assuming 100 g of compound) 1._37.21_ 2._7.83__ 3._54.96_ Moles of element 4.______ 5.______ 6.______ Moles of element/Smallest moles 7.______ 8.______ 9.______ Multiplier 10._____ 10._____ 10.______ Empirical formula 11._____ Molecular weight of empirical formula 12._____ Molecular weight of compound / Molecular weight of empirical formula 13._____
compound has the composition: carbon 37.21%; hydrogen 7.83%; and chlorine 54.96%. If its MW is 385 g/mol, determine (a) the empirical formula (b) the molecular formula. C H Cl Mass of element (in g) (assuming 100 g of compound) 1._37.21_ 2._7.83__ 3._54.96_ Moles of element 4.______ 5.______ 6.______ Moles of element/Smallest moles 7.______ 8.______ 9.______ Multiplier 10._____ 10._____ 10.______ Empirical formula 11._____ Molecular weight of empirical formula 12._____ Molecular weight of compound / Molecular weight of empirical formula 13._____
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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1.
A compound has the composition: carbon 37.21%; hydrogen 7.83%; and chlorine 54.96%. If its MW is 385 g/mol, determine (a) the empirical formula (b) the molecular formula.
| C | H | Cl | |
| Mass of element (in g) (assuming 100 g of compound) | 1._37.21_ | 2._7.83__ | 3._54.96_ |
| Moles of element | 4.______ | 5.______ | 6.______ |
| Moles of element/Smallest moles | 7.______ | 8.______ | 9.______ |
| Multiplier | 10._____ | 10._____ | 10.______ |
| Empirical formula | 11._____ | ||
| Molecular weight of empirical formula | 12._____ | ||
Molecular weight of compound / Molecular weight of empirical formula |
13._____ |
True formula = C12H30Cl6
2.
A hydrocarbon has a MW of 114 g/mol and has a composition of carbon 84.06% and hydrogen 15.94%. What is its (a) empirical formula (b) true formula?
| C | H | |
| Mass of element (in g) (assuming 100 g of compound) | 1._84.06_ | 2._15.94__ |
| Moles of element | 3.______ | 4.______ |
| Moles of element/Smallest moles | 5.______ | 6.______ |
| Multiplier | 7.______ | 7.______ |
| Empirical formula | 8.______ | 9.______ |
| Molecular weight of empirical formula | 10._____ | |
| Molecular weight of compound / Molecular weight of empirical formula | 11._____ |
True formula = C8H18
3.
What is the empirical formula for the compound formed in previous problem?
| Cr | I | |
| Mass of element (in g) | 1. 1.30 g | 2. 9.50 g |
| Moles of element | 3.______ | 4.______ |
| Moles of element/Smallest moles | 5.______ | 6.______ |
| Multiplier | 7.______ | 7.______ |
| Empirical formula | Cr I3 |
4.
Determine the empirical formula of a compound having the following composition: B a = 80.1%, 0 = 18.7%, H = 1.20%.
| B a | O | H | |
| Mass of element (in g) (assuming 100 g of compound) | 1._80.1_ | 2._18.7__ | 3._1.20_ |
| Moles of element | 4.______ | 5.______ | 6.______ |
| Moles of element/Smallest moles | 7.______ | 8.______ | 9.______ |
| Multiplier | 10.______ | 10.______ | 10.______ |
| Empirical formula | Ba(OH)2 |
5.
An organic compound has a gram molecular weight of 372 g/mol, and its composition is 38.6% carbon, 9.76% hydrogen, and 51.56% oxygen. Determine (a) the empirical formula (b) the molecular formula.
| C | H | O | |
| Mass of element (in g) (assuming 100 g of compound) | 1._38.6_ | 2._9.76__ | 3._51.56_ |
| Moles of element | 4.______ | 5.______ | 6.______ |
| Moles of element/Smallest moles | 7.______ | 8.______ | 9.______ |
| Multiplier | 10._____ | 10._____ | 10.______ |
| Empirical formula | 11._____ | ||
| Molecular weight of empirical formula | 12._____ | ||
Molecular weight of compound / Molecular weight of empirical formula |
13._____ |
True formula = C12H36O12
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