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chemistry
organic chemistry

Questions and Answers of Organic Chemistry

Cesium-134 has a half-life of 2.05 y. What is the activity (in curies) of a 0.50-mg sample?
A sample of a phosphorus compound contains phosphorus-32. This sample of radioactive isotope is decaying at the rate of 6.0 × 1012 disintegrations per second. How many grams of 32P are in the
A sample of sodium thiosulfate, Na2S2O3, contains sulfur-35. Determine the mass of 35S in the sample from the decay rate, which was determined to be 7.7 × 1011 disintegrations per second. The
A sample of sodium-24 was administered to a patient to test for faulty blood circulation by comparing the radioactivity reaching various parts of the body. What fraction of the sodium 24 nuclei would
What is a particle accelerator, and how does one operate? Why are they required for certain nuclear reactions?
A solution of sodium iodide containing iodine-131 was given to a patient to test for malfunctioning of the thyroid gland. What fraction of the iodine-131 nuclei would remain undecayed after 7.0 d? If
If 28.0% of a sample of nitrogen-17 decays in 1.97 s, what is the half-life of this isotope (in seconds)?
If 20.0% of a sample of zinc-65 decays in 69.9 d, what is the half-life of this isotope (in days)?
A sample of iron-59 initially registers 125 counts per second on a radiation counter. After 10.0 d, the sample registers 107 counts per second. What is the half-life (in days) of iron-59?
A sample of copper-64 gives a reading of 88 counts per second on a radiation counter. After 9.5 h, the sample gives a reading of 53 counts per second. What is the half-life (in hours) of copper-64?
Carbon from a cypress beam obtained from the tomb of Sneferu, a king of ancient Egypt, gave 8.1 disintegrations of 14C per minute per gram of carbon. How old is the cypress beam? Carbon from living
Carbon from the Dead Sea Scrolls, very old manuscripts found in Israel, gave 12.1 disintegrations of 14C per minute per gram of carbon. How old are the manuscripts? Carbon from living material gives
Several hundred pairs of sandals found in a cave in Oregon were found by carbon-14 dating to be 9.0 × 103 years old. What must have been the activity of the carbon-14 in the sandals in
Some mammoth bones found in Arizona were found by carbon-14 dating to be 1.13 × 104 years old. What must have been the activity of the carbon-14 in the bones in disintegrations per minute per gram?
Find the change of mass (in grams) resulting from the release of heat when 1 mol C reacts with 1 mol O2. C(s) + O2(g) → CO2(g); ∆H = –393.5 kJ
In what major way has the discovery of transuranium elements affected the form of modern periodic tables?
Find the change of mass (in grams) resulting from the release of heat when 1 mol SO2 is formed from the elements. S(s) + O2(g) → SO2(g); ∆H = –297 kJ
Calculate the energy change for the following nuclear reaction (in joules per mole ofGive the energy change in MeV pernucleus. See Table 20.3.
Calculate the change in energy, in joules per mole offor the following nuclear reaction.Give the energy change in MeV pernucleus. See Table 20.3.
Obtain the mass defect (in amu) and binding energy (in MeV) for thenucleus. What is the binding energy (in MeV) per nucleon? See Table 20.3.
Obtain the mass defect (in amu) and binding energy (in MeV) for thenucleus. What is the binding energy (in MeV) per nucleon? See Table 20.3.
Sodium-23 is the only stable isotope of sodium. Predict how sodium-20 will decay and how sodium-26 will decay.
Aluminum-27 is the only stable isotope of aluminum. Predict how aluminum-24 will decay and how aluminum-30 will decay.
A uranium-235 nucleus decays by a series of alpha and beta emissions until it reaches lead 207. How many alpha emissions and how many beta emissions occur in this series of decays?
A thorium-232 nucleus decays by a series of alpha and beta emissions until it reaches lead 208. How many alpha emissions and how many beta emissions occur in this series of decays?
A bismuth-209 nucleus reacts with an alpha particle to produce an astatine nucleus and two neutrons. Write the complete nuclear equation for this reaction.
Describe how a Geiger counter works. How does a scintillation counter work?
A bismuth-209 nucleus reacts with a deuteron to produce a polonium nucleus and a neutron. Write the complete nuclear equation for this reaction.
Complete the following equation by filling in the blank.
Complete the following equation by filling in the blank.
Tritium, or hydrogen-3, is formed in the upper atmosphere by cosmic rays, similar to the formation of carbon-14. Tritium has been used to determine the age of wines. A certain wine that has been aged
The naturally occurring isotope rubidium-87 decays by beta emission to strontium-87. This decay is the basis of a method for determining the ages of rocks. A sample of rock contains 102.1 μg 87Rb
When a positron and an electron collide, they are annihilated and two gamma photons of equal energy are emitted. Calculate the wavelength corresponding to this gamma emission.
When technetium-99m decays to technetium-99, a gamma photon corresponding to an energy of 0.143 MeV is emitted. What is the wavelength of this gamma emission? What is the difference in mass between
Calculate the energy released when 5.00 kg of uranium-235 undergoes the following fission process.The masses of and nuclei are 135.8401 amu and 95.8629 amu, respectively. Other masses are given in
Calculate the energy released when 1.00 kg of hydrogen-1 undergoes fusion to helium-4, according to the following reaction.This reaction is one of the principal sources of energy from the sun.
The half-life of calcium-47 is 4.536 days and it decays by the emission of a beta particle. a. Write a balanced equation for the decay of Ca-47. b. If 10.0 μg of Ca-47 is needed for an experiment,
What is an alloy? Give an example.
Give the commercial source of each of the following metals: Li, Na, Mg, Ca, Al, Sn, Pb.
Complete and balance the following equations.b. Ba(s) + H2O(l) †’c. Mg(OH)2(s) + HNO3(aq) †’d. Mg(s) + NiCl2(aq) †’e. NaOH(aq) + MgSO4(aq) †’
Complete and balance the following equations. a. KOH(aq) + MgCl2(aq) → b. Mg(s) + CuSO4(aq) → c. Sr(s) + H2O(l) → d. SrCO3(s) + HCl(aq) → e. Ba(OH)2(aq) + CO2(g) →
You have a 0.12 M solution of calcium hydrogen carbonate. How many grams of calcium hydroxide must be added to 25.0 mL of the solution to precipitate all of the calcium?
You have a 0.21 M solution of magnesium ion. How many grams of calcium hydroxide must be added to 50.0 mL of the solution to precipitate all of the magnesium ion?
When aluminum sulfate is dissolved in water, it produces an acidic solution. Suppose the pH of this solution is raised by the dropwise addition of aqueous sodium hydroxide. (a) Describe what you
The following solid substances are in separate but unlabeled test tubes: Al2(SO4)3 ∙ 18H2O, BaCl2 ∙ 2H2O, KOH. Describe how you could identify the compounds by chemical tests using only these
Give equations for the reactions of lithium and sodium metals with water and with oxygen in air.
Unlabeled test tubes contain solid AlCl3 ∙ 6H2O in one, Ba(OH)2 ∙ 8H2O in another, and MgSO4 ∙ 7H2O in the other. How could you find out what is in each test tube, using chemical tests that
Lead(IV) oxide is a strong oxidizing agent. For example, lead(IV) oxide will oxidize hydrochloric acid to chlorine, Cl2. Write the balanced equation for this reaction.
Lead(IV) oxide can be prepared by oxidizing plumbiteion, Pb(OH)3 , which exists in a basic solution of Pb2+. Write the balanced equation for this oxidation by OCl in basic solution.
Complete and balance the following equations.a. Al2O3(s) + H2SO4(aq) †’b. Al(s) +AgNO3(aq) †’c. Pb(NO3)2(aq) + NaI(aq) †’d. Al(s) + Mn3O4(s) †’
Complete and balance the following equations. a. Pb(NO3)2(aq) +Al(s) → b. Pb(NO3)2(aq) + Na2CrO4(aq) → c. Al2(SO4)3(aq) + dilute LiOH(aq) → d. Al(s) + HCl(aq) → e. Sn(s) + HBr(aq) →
Calculate the amount of heat evolved when 3.5 × 104 kg of hydrogen is combusted. 2H2(g) + O2(g) → 2H2O(g) ΔH = 484 kJ
How much heat will be evolved when 20.0 grams of the binary covalent hydride HF is produced via the following reaction? F2(g) + H2(g) → 2HF(g) ΔH = 545 kJ
Indicate the oxidation state for the element noted in each ssof the following: a. H in CaH2 b. H in H2O c. C in CH4 d. S in H2SO4
Indicate the oxidation state for the element noted in each of the following: a. H in H2 b. H in C2H4 c. Si in SiH4 d. N in HNO3
Describe the bonding (using valence bond theory) of the Group IVA atoms in each of the following: a. C2H6 b. SiF62 c. CH3CHP==CH2 d. SiH4
Describe the bonding (using valence bond theory) of the Group IVA atoms in each of the following: a. CCl4 b. HCN c. SiF4 d. CH3COOH (acetic acid)
Calculate the standard enthalpy change for the following “cracking” reactions. a. CH4(g) → C(graphite) + 2H2(g) b. C2H6(g) → C2H4(g) + H2(g)
Calculate the standard enthalpy change for the following reactions involving synthesis gas. a. CO(g) + 2H2(g) → CH3OH(g) b. CO(g) + 3H2(g) → CH4(g) + H2O(g)
Silicon has a diamond-like structure, with each Si atom bonded to four other Si atoms. Describe the bonding in silicon in terms of hybrid orbitals.
Which do you expect to be more reactive, lithium or potassium? Explain.
Silicon carbide, SiC, has a structure in which each Si atom is bonded to four C atoms, and each C atom is bonded to four Si atoms. Describe the bonding in terms of hybrid orbitals.
Silicon is prepared by reducing silicon dioxide with carbon at high temperature. How many kilograms of silicon dioxide are required to prepare 5.00 kg of silicon?
Silicon is purified by first converting it to silicon tetrachloride, which is then distilled. How many kilograms of silicon are required to prepare 5.00 kg of SiCl4?
Draw a portion of the structure of the mineral spodumene, LiAl(SiO3)2, which is a mineral consisting of a long chain of SiO4 tetrahedra. Use this drawing to verify the empirical formula given.
Draw a portion of the structure of the mineral beryl, Be3Al2(SiO3)6, which is a mineral consisting of cyclic silicate anions. Use this drawing to verify the empirical formula given.
Magnesium nitride, Mg3N2, reacts with water to produce magnesium hydroxide and ammonia. How many grams of ammonia can you obtain from 7.50 g of magnesium nitride?
Ammonia reacts with oxygen in the presence of a platinum catalyst to give nitric oxide, NO. How many grams of oxygen are required in this reaction to give 3.00 g NO?
You have the following substances: NH3, O2, Pt, and H2O. Write equations for the preparation of N2O from these substances.
Give equations for the preparation of N2O. You can use NaOH, NaNO3, H2SO4, and (NH4)2SO4 (plus H2O). Several steps are required.
Zinc metal reacts with concentrated nitric acid to give zinc ion and ammonium ion. Write the balanced equation for this reaction.
Silver metal reacts with nitric acid to give silver ion and nitric oxide. Write the balanced equation for this reaction.
Although phosphorus pentabromide exists in the vapor phase as PBr5 molecules, in the solid phase the substance is ionic and has the structure [PBr4+]Br. What is the expected geometry of PBr4+?
Although phosphorus pentachloride exists in the vapor phase as PCl5 molecules, in the solid phase the substance is ionic and has the structure [PCl4+][PCl6]. What is the expected geometry of PCl6?
Phosphorous acid, H3PO3, is oxidized to phosphoric acid, H3PO4, by hot, concentrated sulfuric acid, which is reduced to SO2. Write the balanced equation for this reaction.
Phosphorous acid, H3PO3, is oxidized to phosphoric acid, H3PO4, by nitric acid, which is reduced to nitrogen monoxide, NO. Write the balanced equation for this reaction.
According to an analysis, a sample of phosphate rock contains 74.6% Ca3(PO4)2, by mass. How many grams of phosphoric acid, H3PO4, can be obtained from 30.0 g of the phosphate rock according to the
According to an analysis, a sample of phosphate rock contains 71.2% Ca3(PO4)2, by mass. How many grams of calcium dihydrogen phosphate, Ca(H2PO4)2, can be obtained from 10.0 g of phosphate rock from
Write an equation for each of the following. a. Burning of lithium metal in oxygen b. Burning of methylamine, CH3NH2, in excess oxygen (N ends up as N2) c. Burning of diethyl sulfide, (C2H5)2S, in
Write an equation for each of the following. a. Burning of calcium metal in oxygen b. Burning of phosphine, PH3, in excess oxygen c. Burning of ethanolamine, HOCH2CH2NH2, in excess oxygen (N ends up
What are the oxidation numbers of sulfur in each of the following? a. SF6 b. SO3 c. H2S d. CaSO3
(a) Write electrode half-reactions for the electrolysis of fused sodium chloride. (b) Do the same for fused sodium hydroxide. The hydroxide ion is oxidized to oxygen and water.
What are the oxidation numbers of sulfur in each of the following? a. S8 b. CaS c. CaSO4 d. SCl4
Selenous acid, H2SeO3, is reduced by H2S to sulfur, S8, and selenium, Se8. Write the balanced equation for this reaction.
Sodium hydrogen sulfite is prepared from sodium carbonate and sulfur dioxide: Na2CO3(s) + 2SO2(g) + H2O(l) → 2NaHSO3(aq) + CO2(g) How many grams of NaHSO3 can be obtained from 25.0 g of Na2CO3?
Sodium thiosulfate, Na2S2O3, is prepared from sodium sulfite and sulfur: 8Na2SO3(aq) + S8(s) → 8Na2S2O3(aq) How many grams of Na2S2O3 can be obtained from 50.0 g of sulfur?
Chlorine can be prepared by oxidizing chloride ion (from hydrochloric acid) with potassium dichromate, K2Cr2O7, which is reduced to Cr3+. Write the balanced equation for the reaction.
Iodic acid, HIO3, can be prepared by oxidizing elemental iodine with concentrated nitric acid, which is reduced to nitrogen dioxide, NO2(g). Write the balanced equation for the reaction.
Discuss the bonding in each of the following molecules or ions. What is the expected molecular geometry? a. Cl2O b. BrO3– c. BrF3
Discuss the bonding in each of the following molecules or ions. What is the expected molecular geometry? a. HClO b. ClO4– c. ClF5
Write balanced equations for each of the following.a. Bromine reacts with aqueous sodium hydroxide to give hypobromite and bromide ions.b. Hydrogen bromide gas forms when sodium bromide is heated
Write balanced equations for each of the following. a. Solid calcium fluoride is heated with sulfuric acid to give hydrogen fluoride vapor. b. Solid potassium chlorate is carefully heated to yield
By calculating the standard emf, decide whether aqueous sodium hypochlorite solution will oxidize Fe2+ (aq) to Fe3+ (aq) in basic solution under standard conditions. See Appendix I for data.
Using standard electrode potentials, decide whether aqueous sodium hypochlorite solution will oxidize Br to Br2 in basic solution under standard conditions. See Appendix I for data.
Xenon tetrafluoride, XeF4, is a colorless solid. Give the Lewis formula for the XeF4 molecule. What is the hybridization of the xenon atom in this compound? What geometry is predicted by the VSEPR
Xenon tetroxide, XeO4, is a colorless, unstable gas. Give the Lewis formula for the XeO4 molecule. What is the hybridization of the xenon atom in this compound? What geometry would you expect for
Xenon difluoride, XeF2, is hydrolyzed (broken up by water) in basic solution to give xenon, fluoride ion, and O2 as products. Write a balanced equation for the reaction.
Xenon trioxide, XeO3, is reduced to xenon in acidic solution by iodide ion. Iodide ion is oxidized to iodine, I2. Write a balanced chemical equation for the reaction.
A sample of zinc ore contains 87.0% sphalerite, ZnS. How many metric tons of Zn can be obtained from 1.00 metric ton of the zinc ore?
Describe common uses of the following sodium compounds: sodium chloride, sodium hydroxide, and sodium carbonate.

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