Concept explainers
(a)
Interpretation:
Mass of water in
Concept Introduction:
Mass percent is one of the commonly used concentration terms to determine concentration of any species. The expression for mass percent of any species present in sample is as follows:
(a)
Answer to Problem 19PE
Mass of water in
Explanation of Solution
Molecular mass of
Substitute 7 for number of molecules of water and
The formula to calculate mass percent of water is as follows:
Substitute
Hence, mass percent of water in
The formula to calculate mass of water is as follows:
Substitute
Hence, mass of water in
(b)
Interpretation:
Mass of anhydrous compound of
Concept Introduction:
Compound that does not contain any water molecule is termed as anhydrous compound. Mass of anhydrous compound is calculated as follows:
(b)
Answer to Problem 19PE
Mass of anhydrous compound is
Explanation of Solution
The expression used to calculate mass of anhydrous compound is as follows:
Substitute
Hence, mass of anhydrous compound is
Want to see more full solutions like this?
Chapter 13 Solutions
FOUND.OF COLLEGE CHEMISTRY
- When one mole of ethylene gas, C2H4, reacts with fluorine gas, hydrogen fluoride and carbon tetrafluoride gases are formed and 2496.7 kJ of heat are given off. What is Hf for CF4(g)?arrow_forwardThe carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forwardWhen calcium carbonate is heated strongly, it evolves carbon dioxide gas. CaCO3(s)CaO(s)+CO2(g) 25 g of CaCO3 is heated, what mass of CO2would be produced? What volume would this quantity of CO2 (CU at STP?arrow_forward
- A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forwardIn the early days of automobiles, illumination at night was provided by burning acetylene, C2H2. Though no longer used as auto headlamps, acetylene is still used as a source of light by some cave explorers. The acetylene is (was) prepared in the lamp by the reaction of water with calcium carbide, CaC2:CaC2(s) + 2H2 O(l) ⟶ Ca(OH)2(s) + C2 H2(g).Calculate the standard enthalpy of the reaction. The ΔH°f of CaC2 is −15.14 kcal/mol.arrow_forward(1) One of the steps in the commercial process for converting ammonia to nitric acid involves the conversion of ammonia, NH3(g) to nitrous oxide, NO(g). 4 NH3(g ) + 5 O2(g) → 4 NO(g) + 6 H2O(l) Atomic weights (g/mol): N=14, H=1, O=16 a. Balance the above chemical equation that represents the conversion. b. How many moles of oxygen are needed to convert 2.5 moles of ammonia? c. How many grams of water will be produced from 2.5 moles of ammonia? d. If 150 grams of oxygen reacted 2.5 moles of ammonia, identify the limiting and excess reagents. e. How much of the excess reagent remains unreacted? f. If the reaction in (d) produces 10.0 grams of nitrous oxide, calculate the percent yield.arrow_forward
- When active metals such as sodium are exposed to air, they quickly form a coating of metal oxide. The balanced equation for the reaction of sodium metal with oxygen gas is 4Na(s) + O₂(g) 2Na₂O(s) Suppose a piece of sodium metal gains 2.05 g of mass after being exposed to air. Assume that this gain can be attributed to its reaction with oxygen. (a) What mass of O₂ reacted with the Na? (b) What mass of Na reacted? (c) What mass of Na₂O formed? 01.0arrow_forwardThe reaction of pentane, C5H12, with oxygen, O2, gives carbon dioxide and water. (a) Write a balanced equation for this reaction.arrow_forwardWrite chemical equations for each of the following chemical and physical processes: (a) Reaction of ammonia gas with hydrogen chloride gas to produce a solid product (b) Reaction of 1 mole of aluminum with I2(s) to form aluminum iodide (c) Conversion of 1 mole of O2(g) to O3(g) (d) Dissolving K2Cr2O7(s) in water (e)Thermal decomposition of solid sodium azide to produce solid sodium and nitrogen gas (f) Photodissociation of chlorine gas (g) Fusion of icearrow_forward
- CO, H2 → CH, H,O (a) How many moles of water can be produced from 25 moles of carbon dioxide? (a (b) How many moles of CH4 will be produced along with 12 (b moles of water?arrow_forwardAluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. (a) Write a balanced equation for this reaction. (b) How many grams of aluminum hydroxide can be obtained from 5.50 g of aluminum sulfide?arrow_forwardDecane, C10H22(l), undergoes complete combustion if there is sufficient oxygen available: 2 C10H22(l) + 31 O2(g) → 20 CO2(g) + 22 H2O(g) (a) What mass of oxygen is required for the complete combustion of 800g of decane? (b) A sample of decane is burned, producing 12 mol of carbon dioxide. What amount (moles) of water is also produced? Include a therefore statement for EACH a) and b)arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning