Concept explainers
(a)
Interpretation:
The percent by mass of element listed first in the formula of a compound should be calculated.
Concept Introduction:
A chemical compound is a collection of several atoms. Molar masses of each and every atom collectively provide the molar mass of that compound.
Mass fraction for a given element can be converted into mass percent by multiplying
Answer to Problem 49QAP
Explanation of Solution
The compound is adipic acid,
Molar mass of carbon is 12.01 g/mol, hydrogen is 1.008 g/mol and oxygen is 16.0 g/mol.
Thus, the molar mass of adipic acid can be calculated as follows:
Now, mass of carbon in 1 mol is 12.01 g thus, mass of 6 mol of carbon will be:
Mass of adipic acid in 1 mol is 146.14 g.
Thus, mass percent of C can be calculated as follows:
(b)
Interpretation:
The percent by mass of element listed first in the formula of a compound should be calculated.
Concept Introduction:
A chemical compound is a collection of several atoms. Molar masses of each and every atom collectively provide the molar mass of that compound.
Mass fraction for a given element can be converted into mass percent by multiplying
Answer to Problem 49QAP
Explanation of Solution
The compound is ammonium nitrate
Molar mass of nitrogen is 14 g/mol, hydrogen is 1.008 g/mol and oxygen is 16.0 g/mol.
Thus, the molar mass of ammonium nitrate can be calculated as follows:
Now, mass of nitrogen in 1 mol is 14 g thus, mass of nitrogen in 2 mol is 28 g.
Mass of ammonium nitrate in 1 mol is 80.043 g.
Thus, mass percent of N can be calculated as follows:
(c)
Interpretation:
The percent by mass of element listed first in the formula of a compound should be calculated.
Concept Introduction:
A chemical compound is a collection of several atoms. Molar masses of each and every atom collectively provide the molar mass of that compound.
Mass fraction for a given element can be converted into mass percent by multiplying
Answer to Problem 49QAP
Explanation of Solution
The compound is caffeine
Molar mass of carbon is 12.01 g/mol, hydrogen is 1.008 g/mol, nitrogen is 14 g/mol and oxygen is 16.0 g/mol.
Thus, the molar mass of caffeine can be calculated as follows:
Now, mass of carbon in 1 mol is 12.01 g thus, mass of carbon in 8 mol will be:
Mass of caffeine in 1 mol is 194.2 g.
Thus, mass percent of C can be calculated as follows:
(d)
Interpretation:
The percent by mass of element listed first in the formula of a compound should be calculated.
Concept Introduction:
A chemical compound is a collection of several atoms. Molar masses of each and every atom collectively provide the molar mass of that compound.
Mass fraction for a given element can be converted into mass percent by multiplying
Answer to Problem 49QAP
Explanation of Solution
The compound is chlorine dioxide
Molar mass of chlorine is 35.5 g/mol and oxygen is 16.0 g/mol.
Thus, the molar mass of chlorine dioxide can be calculated as follows:
Now, mass of chlorine in 1 mol is 35.5 g and mass of chlorine dioxide in 1 mol is 67.5 g.
Thus, mass percent of Cl can be calculated as follows:
(e)
Interpretation:
The percent by mass of element listed first in the formula of a compound should be calculated.
Concept Introduction:
A chemical compound is a collection of several atoms. Molar masses of each and every atom collectively provide the molar mass of that compound.
Mass fraction for a given element can be converted into mass percent by multiplying
Answer to Problem 49QAP
Explanation of Solution
The compound is cyclohexanol
Molar mass of carbon is 12.01 g/mol, molar mass of hydrogen is 1.008 g/mol and oxygen is 16.0 g/mol.
Thus, the molar mass of cyclohexanol can be calculated as follows:
Now, mass of carbon in 1 mol is 12.01 g thus, mass of carbon in 6 mol is 72.06 g.
Mass of cyclohexanol in 1 mol is 100.16 g.
Thus, mass percent of C can be calculated as follows:
(f)
Interpretation:
The percent by mass of element listed first in the formula of a compound should be calculated.
Concept Introduction:
A chemical compound is a collection of several atoms. Molar masses of each and every atom collectively provide the molar mass of that compound.
Mass fraction for a given element can be converted into mass percent by multiplying
Answer to Problem 49QAP
Explanation of Solution
The compound is dextrose
Molar mass of carbon is 12.01 g/mol, molar mass of hydrogen is 1.008 g/mol and oxygen is 16.0 g/mol.
Thus, the molar mass of dextrose can be calculated as follows:
Now, mass of carbon in 1 mol is 12.01 g thus, mass of carbon in 6 mol is 72.06 g.
Mass of cyclohexanol in 1 mol is 100.16 g.
Thus, mass percent of C can be calculated as follows:
(g)
Interpretation:
The percent by mass of element listed first in the formula of a compound should be calculated.
Concept Introduction:
A chemical compound is a collection of several atoms. Molar masses of each and every atom collectively provide the molar mass of that compound.
Mass fraction for a given element can be converted into mass percent by multiplying
Answer to Problem 49QAP
Explanation of Solution
The compound is eicosane
Molar mass of carbon is 12.01 g/mol and molar mass of hydrogen is 1.008 g/mol.
Thus, the molar mass of eicosane can be calculated as follows:
Now, mass of carbon in 1 mol is 12.01 g thus, mass of carbon in 20 mol is 240.2 g.
Mass of eicosane in 1 mol is 282.55 g.
Thus, mass percent of C can be calculated as follows:
(h)
Interpretation:
The percent by mass of element listed first in the formula of a compound should be calculated.
Concept Introduction:
A chemical compound is a collection of several atoms. Molar masses of each and every atom collectively provide the molar mass of that compound.
Mass fraction for a given element can be converted into mass percent by multiplying
Answer to Problem 49QAP
Explanation of Solution
The compound is ethanol
Molar mass of carbon is 12.01 g/mol molar mass of oxygen is 16.0 g/mol and molar mass of hydrogen is 1.008 g/mol.
Thus, the molar mass of ethanol can be calculated as follows:
Now, mass of carbon in 1 mol is 12.01 g thus, mass of carbon in 2 mol is 24.02 g.
Mass of ethanol in 1 mol is 46.1 g.
Thus, mass percent of C can be calculated as follows:
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Chapter 8 Solutions
Student Solutions Manual For Zumdahl/decoste's Introductory Chemistry: A Foundation, 8th Edition
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- Two general chemistry students working together in the lab weigh out 0.832 g of CaCl2 2 H2O into a crucible. After heating the sample for a short time and allowing the crucible to cool, the students determine that the sample has a mass of 0.739 g. They then do a quick calculation. On the basis of this calculation, what should they do next? (a) Congratulate themselves on a job well done. (b) Assume the bottle of CaCl2 2 H2O was mislabeled; it actually contained something different. (c) Heat the crucible again, and then reweigh it.arrow_forwardExpress the composition of each of the following compounds as the mass percents of its elements. a. formaldehyde, CH2O b. glucose, C6H12O6 c. acetic acid, HC2H3O2arrow_forward
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