(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 20PE
Mass of water in
Explanation of Solution
Molecular mass of
Substitute 6 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 20PE
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
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Chapter 13 Solutions
EBK FOUNDATIONS OF COLLEGE CHEMISTRY
- The 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_forwardEthanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.arrow_forward4.19 How many metric tons of carbon are required to react with 7.83 metric tons of Fe2O3 according to the following reaction? 2Fe2O3+3C3CO2+4Fe How many metric tons of iron are produced?arrow_forward
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- (1) Hydrofluoric acid, HF(aq), cannot be stored in glass bottles because compounds called silicates in the glass are attacked by the HF(aq). For example, sodium silicate, Na2SiO3, reacts in the following way Na2SiO3(s) + 8 HF(aq) → H2SiF6 (aq) + 2 NaF(aq) + 3 H2O(l) Atomic weights (g/mol): Na=23, Si=28, O=16, H=1, F=19 (a) Balance the above chemical equation that represents the reaction. (b) How many moles of sodium silicate can be attacked by 9.0 moles of hydrofluoric acid? (c) How much each (in grams) of NaF(aq) and water will be produced from 9.0 moles of hydrofluoric acid? (d) If 200 grams of HF(aq) attacked 1.5 moles sodium silicate , identify the limiting and excess reagents (e) How much of the excess reagent remains unreacted? (f) If the reaction in (d) produces 40.0 grams of NaF, calculate the percent yield.arrow_forwardWrite “true” or “false” for each statement. (a) We balancechemical equations as we do because energy must be conserved.(b) If the reaction 2 O3(g)S 3 O2(g) goes to completionand all O3 is converted to O2, then the mass of O3 atthe beginning of the reaction must be the same as the massof O2 at the end of the reaction. (c) You can balance the“water-splitting” reaction H2O(l)S H2(g) + O2(g) by writingit this way: H2O2(l)S H2(g) + O2(g).arrow_forwardCitric acid (C6H8O7) is made by fermentation of sugars such as sucrose (C12H22O11) in air. Oxygen is consumed and water generated as a by-product.(a) Write a balanced equation for the overall reaction that occurs in the manufacture of citric acid from sucrose.(b) What mass of citric acid is made from 15.0 kg sucrose?arrow_forward
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