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(a)
Interpretation: The electron dot structures for ethanol, ethylamine, acetonitrile, and acrylonitrile have to be drawn, molecular geometry around the central atom in these molecules should be determined.
Concept introduction:
Lewis dot structure: For a given molecule, the bonding concerning the atoms and also the lone pairs can be shown by a diagram.
In this structure a single bond is represented by one dot pair and double bond is represented by two dot pairs and so on.
VSEPR Theory [Valence Shell Electron Pair Repulsion Theory]:
Geometry of the molecules can be predicted using VSEPR Theory. It is based on the number of electron pairs around the central atom of the molecule. Depending upon the bond pairs and lone pairs, geometries can be classified as linear, bent, pyramidal, and trigonal planar, tetrahedral, and octahedral and so on.
(b)
Interpretation: The balanced equations for each step in the synthesis of acetonitrile from ethanol should be written.
Concept introduction:
- For
chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass. - Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
- Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.
(c)
Interpretation: Atom economy for the synthesis of acetonitrile from ethanol should be determined.
Concept introduction:
Atom economy: The amount of mass of reactants which is converted into useful products.
Atom economy
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Chapter 20 Solutions
Chemistry & Chemical Reactivity
- 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_forwardA 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_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_forward
- Although the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat produced by combustion of one mole of acetylene in such a torch is likely not equal to the enthalpy of combustion of acetylene listed in Table 5.2. Considering the conditions for which the tabulated data are reported, suggest an explanation.arrow_forwardUse the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.arrow_forwardThe heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)arrow_forward
- 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_forwardBalance the following chemical equation (ifnecessary):C6H6O(I) + O2(g) -> H20 (g) + CO2 (g)arrow_forwardOne method for chemical analysis involves finding a reactant that will precipitate the species of interest, but not the other species. The mass of the precipitate is then used to determine the mass of the species of interest present in the original sample. For example, calcium ions can be precipitated from an aqueous solution by adding of sodium oxalate Na2C2O4. The balanced equation is: Ca2+(aq) + Na2C2O4 (aq) --> CaC2O4 (s) + 2 Na+ (aq) Suppose you had a solution with approximately 15.0 g of calcium ions. Show by calculation whether the addition of 15.0 g of sodium oxalate will precipitate all of the calcium ions present in the sample.arrow_forward
- Although we tend to make less use of mercury these days because of the environmental problems created by its improper disposal, mercury is still an important metal because of its unusual property of existing as a liquid at room temperature. One process by which mercury is produced industrially is through the heating of its common ore cinnabar (mercuric sulfide, HgS) with lime (calcium oxide, CaO). 4 HgS(s) + 4 CaO(s) → 4 Hg(l) + 3 CaS(s) + CaSO4(s) What mass of mercury would be produced by complete reaction of 10.7 kg of HgS? kgarrow_forwardNitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by réforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N2(9)+3 H,(g)→2NH;(g) In the second step, ammonia and oxygen react to form nitric acid and water: NH;(g)+2O,(9)→HNO,(g)+H,O(g) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced. Explanation Check O2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility 2:53 PM 4/8/2022 DELL PrtScr Insert Delete PgUp PgDn F7 F8 F9 F10 F11 F12 Esc F1 F2 F3 F4 F5 F6 Fn Num 24 & ( ) Lock Backspace 1 2 6. 7 + II * 00 %#3arrow_forwardThe psychoactive drug methamphetamine ("speed"), which is sold as the prescription medication Desoxyn, C10H15N, under- goes a series of reactions in the body; the net result of these reac- tions is the oxidation of solid methamphetamine by oxygen gas to produce carbon dioxide gas, liquid water, and an aqueous solution of urea, CH4N₂O. Write the balanced equation for this net reaction.arrow_forward
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