Concept explainers
(a)
Interpretation:
The percent composition of nitrogen in
(a)
Explanation of Solution
The percent composition of any substance is calculated by dividing the mass of the substance in a sample by the total mass of the sample. This ratio is multiplied by
To determine the percent composition, let the
The mass of Na from the periodic table is
The mass of N from the periodic table is
The mass of O from the periodic table is
Therefore, the total mass of
Now, the percent composition of N is as follows:
(b)
Interpretation:
The percentage of nitrogen in
(b)
Explanation of Solution
To determine the percent composition, let the sample size be
The mass of N from the periodic table is
The mass of H from the periodic table is
The mass of Cl from the periodic table is
Therefore, the total mass of
Now, the percent composition of N is as follows:
(c)
Interpretation:
The percentage of nitrogen in
(c)
Explanation of Solution
To determine the percent composition, let the sample size be
The mass of N from the periodic table is
The mass of H from the periodic table is
Therefore, the total mass of
Now, the percent composition of N is as follows:
(d)
Interpretation:
The percentage of nitrogen in
(d)
Explanation of Solution
To determine the percent composition, let the sample size be
The mass of N from the periodic table is
The mass of O from the periodic table is
Therefore, the total mass of
Now, the percent composition of N is as follows:
Want to see more full solutions like this?
Chapter 4 Solutions
INTO TO CHEMISTRY (EBOOK ACCESS CODE)
- The sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. C12H22O11(aq) + H2O(l) C2H5OH(aq) + CO2(g)arrow_forwardHow many moles of nitrogen atoms are present in 3.00-mole samples of each of the following compounds? a. S2N2 b. S4N4 c. NSF d. N4S4Cl4arrow_forwardHow many moles of specified particles are present in a sample of each of the following substances if each sample weighs 5.00 g? a. CO molecules b. CO2 molecules c. B4H10 molecules d. U atomsarrow_forward
- Balance each of the following chemical equations. a. KO2(s) + H2O(l) KOH(aq) + O2(g) + H2O2(aq) b. Fe2O3(s) + HNO3(aq) Fe(NO3)(aq) + H2O(l) c. NH3(g) + O2(g) NO(g) + H2O (g) d. PCl5(l) + H2O(l) H3PO4(aq) + HCl(g) e. CaO(s) + C(s) CaC2(s) + CO2 (g) f. MoS2(s) + O2(g) MoO3(s) + SO2 (g) g. FeCO3(s) + H2CO3(aq) Fe(HCO3)2(aq)arrow_forwardBalance these equations. (a) UO2(s) + HF() UF4(s) + H2O() (b) B2O3(s) + HF() BF3(g) + H2O() (c) BF3(g) + H2O() HF() + H3BO3(s)arrow_forwardA 0509-g sample of an unknown organic compound containing C, H, and O was burned in air to give 1.316 g of CO2 and 0.269 g of H2O. What is the empirical formula for this compound? (a) CHO (b) C2H2O (c) C4H4O (d) CHO4arrow_forward
- Calculate the molar mass of the following substances. a. b. c. (NH4)2Cr2O7arrow_forwardCalculate the molar mass of the following substances. a. b. Ca3(PO4)2 c. Na2HPO4arrow_forwardQuicklime, CaO, is formed when calcium hydroxide is heated. Ca(OH)2(s) → CaO(s) + H2O(ℓ) The theoretical yield is 65.5 g but only 36.7 g quicklime I is produced. Calculate the percent yield.arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning