General Chemistry 9th edition Darrell Ebbing, Steven D. Gammon - Solutions

Methyl chloride, CH3Cl, reacts in basic solution to give methanol.This reaction is believed to occur in a single step. If so, what should be the rate law? CH;CI + OH - CH,ОН + CI
At high temperature, the reactionis thought to occur in a single step. What should be the rate law in that case? NO2(8) + CO(g) NO(8) + CO2(8)
What is the molecularity of each of the following elementary reactions?a. O + O2 + N2 → O3 + N*2b. NO2Cl + Cl → NO2 + Cl2c. Cl + H2 → HCl + Hd. CS2 → CS + S
Identify the molecularity of each of the following elementary reactions.a. NO + O3 → NO2 + O2b. NOCl2 + NO → 2NOClc. O3 → O2 + Od. H + H + N2 → H2 + N*2
You carry out the following reaction by introducing N2O4 into an evacuated flask and observing the concentration change of the product over time.N2O4(g) → 2NO2(g)Which one of the curves shown here reflects the data collected for this reaction? Curve A Curve B Time (s) → Time (s) - Curve C Curve
Given the reaction 2A + B → C + 3D, can you write the rate law for this reaction? If so, write the rate law; if not, why?
The hypothetical reactionA + B + C → D + Ehas the rate law Rate = k[A]2[B]. Which of the following changes would have the least effect on increasing the rate of this reaction?a. Doubling [A]0 while keeping [B]0 and [C]0 constant.b. Doubling [B]0 while keeping [A]0 and [C]0 constant.c.
At a constant temperature, which of the following would be expected to affect the rate of a given chemical reaction, A + B → C + D?I. The reaction temperatureII. The concentration of the productsIII. A catalysta. I onlyb. II onlyc. III onlyd. I and II onlye. I and III only
At a constant temperature, which of the following would be expected to affect the rate of a given chemical reaction, A + B → C + D?I. The reaction temperatureII. The concentration of the productsIII. A catalysta. I onlyb. II onlyc. III onlyd. I and II onlye. I and III only
You are running the reaction 2A + B → C + 3D. Your lab partner has conducted the first two experiments to determine the rate law for the reaction by the method of initial rates.Presuming that you can measure the initial rate of each experiment, which of the following concentrations for Experiment
You are running the reaction 2A + B → C + 3D. Your lab partner has conducted the first two experiments to determine the rate law for the reaction by the method of initial rates.
Compare physical adsorption and chemisorption (chemical adsorption).
Aluminum hydroxide forms a positively charged sol. Which of the following ionic substances should be most effective in coagulating the sol?a. NaClb. CaCl2c. Fe2(SO4)3d. K3PO4
Arsenic(III) sulfide forms a sol with a negative charge. Which of the following ionic substances should be most effective in coagulating the sol?a. KClb. MgCl2c. Al2(SO4)3d. Na3PO4
Which of the following ions would be expected to have the greater energy of hydration, F or Cl?
Which of the following ions would be expected to have the greater energy of hydration, Mg2+ or Al3+?
Arrange the following substances in order of increasing solubility in hexane, C6H14: CH2OHCH2OH, C10H22, H2O.
Would naphthalene, C10H8, be more soluble in ethanol, C2H5OH, or in benzene, C6H6?
Would boric acid, B(OH)3, be more soluble in ethanol, C2H5OH, or in benzene, C6H6?
Give an example of a solid solution prepared from two solids.
Give an example of a liquid solution prepared by dissolving a gas in a liquid.
People have proposed towing icebergs to arid parts of the earth as a way to deliver freshwater. Explain why icebergs do not contain salts although they are formed by the freezing of ocean water (i.e., saltwater).
A 5.1-g sample of CaCl2 is dissolved in a beaker of water. Which of the following statements is true of this solution?a. The solution will freeze at a lower temperature than pure water.b. The solution has a higher vapor pressure than pure water.c. The solution will boil at a lower temperature than
If 291g of a compound is added to 1.02 kg of water to increase the boiling point by 5.77°C, what is the molar mass of the added compound? (Assume a van’t Hoff factor of 1.)a. 31.1 g/molb. 30.3 g/molc. 28.5 g/mold. 18.3 g/mole. 25.3 g/mol
The mole fraction of copper(II) nitrate in an aqueous copper(II) nitrate solution is 0.135. What is the molality of the copper(II) nitrate solution?a. 7.49 mb. 8.01 mc. 8.66 md. 9.34 me. 8.09 m
Calculate the number of moles of barium chloride in 427 g of a 3.17% by mass barium chloride solution?a. 6.50 × 1002 molb. 7.83 × 1002 molc. 4.31 × 1002 mold. 7.81 × 1002 mole. 4.27 × 1002 mol
Give an example of an aerosol, a foam, an emulsion, a sol, and a gel.
What do you expect to happen to a concentration of dissolved gas in a solution as the solution is heated?
What famous chemist first predicted the greenhouse effect of carbon dioxide gas?
How does nitroglycerine alleviate the pain of an angina attack?
A 1-liter container is filled with 2.0 mol Ar, 2.0 mol H2, and 4.0 mol Kr. Which of the following statements about these gases is false? a. The Kr is the densest of the three gases. b. The mole fraction of Ar in the flask is 0.25. c. The total pressure in the flask is four times the
At standard temperature and pressure, a 1.00-mol sample of argon gas is vented into a 22.4-L rigid box that already contains 1.00 mol of nitrogen gas. We would expect the argon gas to a. decrease the total gas pressure in the box by 50%. b. occupy the entire 22.4-L volume of the
A sample of nitrogen gas is placed into a container at 200 K. If the temperature of the container is reduced by 100C and the measured pressure decreases by 50%, how does the volume of the container change? a. The container volume increases by less than 50%. b. The container volume
Which of the following is not part of the kinetic molecular theory? a. The greater the volume occupied by a given amount of gas, the higher the intermolecular forces. b. The average kinetic energy is proportional to the absolute temperature. c. Gas particles are in constant
What is the physical meaning of the a and b constants in the van der Waals equation?
Under what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?
How does the rms molecular speed depend on absolute temperature? on molar volume?
What is the origin of gas pressure, according to kinetic theory?
What variables are needed to describe a gas that obeys the ideal gas law? What are the SI units for each variable?
What does the term molar gas volume mean? What is the molar gas volume (in liters) at STP for an ideal gas?
What are the standard conditions for comparing gas volumes?
Part 1 a. Both NaCl and MgCl2 are soluble ionic compounds. Write the balanced chemical equations for these two substances dissolving in water. b. Consider the pictures below. These pictures represent 1.0-L solutions of 1.0 M NaCl(aq) and 1.0 M MgCl2(aq). The representations of the ions in
Part 1a. Ammonia, NH3, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols. b. From everyday experience you are probably aware that table
What is the volume (in milliliters) of 0.215 M H2SO4 (sulfuric acid) containing 0.949 g H2SO4?
An experiment calls for 0.0353 g of potassium hydroxide, KOH. How many milliliters of 0.0176 M KOH are required?
How many milliliters of 0.126 M HClO4 (perchloric acid) are required to give 0.102 mol HClO4?
What volume of 0.120 M CuSO4 is required to give 0.150 mol of copper(II) sulfate, CuSO4?
Write the molecular equation and the net ionic equation for the reaction of solid barium carbonate and hydrogen bromide in aqueous solution. Add phase labels.
Write the molecular equation and the net ionic equation for the reaction of solid iron(II) sulfide and hydrochloric acid. Add phase labels.
Potassium carbonate solution reacts with aqueous hydrobromic acid to give a solution of potassium bromide, carbon dioxide gas, and water. Write the molecular equation and the net ionic equation for the reaction.
Lead(II) nitrate solution and sodium sulfate solution are mixed. Crystals of lead(II) sulfate come out of solution, leaving a solution of sodium nitrate. Write the molecular equation and the net ionic equation for the reaction.
Would you expect a precipitation reaction between an ionic compound that is an electrolyte and an ionic compound that is a nonelectrolyte? Justify your answer.
Three acid samples are prepared for titration by 0.01 M NaOH: 1. Sample 1 is prepared by dissolving 0.01 mol of HCl in 50 mL of water. 2. Sample 2 is prepared by dissolving 0.01 mol of HCl in 60 mL of water. 3. Sample 3 is prepared by dissolving 0.01 mol of HCl in 70 mL of
In an aqueous 0.10 M HNO2 solution (HNO2 is a weak electrolyte), which of the following would you expect to see in the highest concentration? a. H3O+ b. NO2- c. H+ d. HNO2 e. OH-
Which of the following compounds would produce the highest concentration of Cl- ions when 0.10 mol of each is placed in separate beakers containing equal volumes of water? a. NaCl b. PbCl2 c. HClO4 d. MgCl2 e. HCl
An aqueous sodium hydroxide solution mixed with an aqueous magnesium nitrate solution yields which of the following products? a. Magnesium hydroxide(aq) b. Magnesium dihydroxide(s) c. Magnesium hydroxide(s) d. Dimagnesium hydroxide(s) e. sodium nitrate(l)
What is the net ionic equation for the following molecular equation? Hydrofluoric acid, HF, is a molecular substance and a weak electrolyte. HF(aq) + KОH(ад) — KFaq) + Н.О()
Why is the product of molar concentration and volume constant for a dilution problem?
Why must oxidation and reduction occur together in a reaction?
When 2.56 g of a compound containing only carbon, hydrogen, and oxygen is burned completely, 3.84 g of CO2 and 1.05 g of H2O are produced. What is the empirical formula of the compound? a. C3H4O3 b. C5H6O4 c. C5H6O5 d. C4H4O3 e. C4H6O3
How many atoms are present in 123 g of magnesium cyanide? a. 9.7 × 1023 b. 2.91 × 1024 c. 2.83 × 1028 d. 4.85 × 1024 e. 5.65 × 1027
How many atoms are present in 123 g of magnesium cyanide? a. 9.7 × 1023 b. 2.91 × 1024 c. 2.83 × 1028 d. 4.85 × 1024 e. 5.65 × 1027
Which of the following has the largest number of molecules? a. 1 g of benzene, C6H6 b. 1 g of formaldehyde, CH2O c. 1 g of TNT, C7H5N3O6 d. 1 g of naphthalene, C10H8 e. 1 g of glucose, C6H12O6
Which of the following has the largest number of molecules? a. 1 g of benzene, C6H6 b. 1 g of formaldehyde, CH2O c. 1 g of TNT, C7H5N3O6
How many grams of NH3 will have the same number of molecules as 15.0 g of C6H6? a. 3.27 b. 1.92 c. 15.0 d. 17.0 e. 14.2
Describe in words how to obtain the formula mass of a compound from the formula.
Ammonia gas reacts with molecular oxygen gas to form nitrogen monoxide gas and liquid water. Write the complete balanced reaction with all proper state symbols.
An unknown metal (let’s call it “M”) is reacted with sulfur to produce a compound with the chemical formula M2S3. What is the charge on the metal in the compound M2S3? Name a metal that could be metal M.
Write the equation for the nuclear reaction in which element 112 was first produced.
Write formulas for all the ionic compounds that can be formed by combinations of these ions: Ca2+, Cr3+, O2-, and NO3-.
Write formulas for all the ionic compounds that can be formed by combinations of these ions: Na+, Ni2+, SO42-, and Cl-.
Cobalt(II) chloride hexahydrate has a pink color. It loses water on heating and changes to a blue-colored compound. What is the formula of cobalt(II) chloride hexahydrate?
Iron(II) sulfate heptahydrate is a blue-green, crystalline compound used to prepare other iron compounds. What is the formula of iron(II) sulfate heptahydrate?
Emerald-green crystals of the substance NiSO4•6H2O are used in nickel plating. What is the chemical name of this compound?
Glauber’s salt has the formula Na2SO4•10H2O. What is the chemical name of this substance?
Write the systematic name for each of the following molecules represented by a molecular model. a.b.c. FC
Write the systematic name for each of the following compounds represented by a molecular model. a.b.c. Se
Refer to the periodic table (Figure 2.15 or inside front cover) and answer the following questions. a. What Group VA element is a metal? b. What is the Group IIA element in Period 3? Figure 2.15 Main-Group Elements Main-Group Elements 1 Atomic number 18 IA Symbol Atomic mass H VIIА
Refer to the periodic table (Figure 2.15 or inside front cover) and answer the following questions. a. What Group VIA element is a metalloid? b. What is the Group III A element in Period 3?Figure 2.15 Main-Group Elements Main-Group Elements 1 Atomic number 18 IA Symbol Atomic mass H VIIА
An atom contains 11 protons and 11 neutrons. What is the nuclide symbol for the nucleus?
What is the nuclide symbol for the nucleus that contains 14 protons and 14 neutrons?
The following table gives the number of protons and neutrons in the nuclei of various atoms. Which atom is the isotope of atom A? Which atom has the same mass number as atom A? Protons Neutrons Atom A 32 39 Atom B 32 38 Atom C 38 50 Atom D 33 38
The following table gives the number of protons and neutrons in the nuclei of various atoms. Which atom is the isotope of atom A? Which atom has the same mass number as atom A? Protons Neutrons Atom A 18 19 Atom B 16 19 Atom C 18 18 Atom D 17 20
The following table gives the number of protons and neutrons in the nuclei of various atoms. Which atom is the cases, the reactants are elements and the products are binary compounds a. LICI b. Na,S C. Al Br2 d. Mg N2 е. Ca P2 + + + + +
Given that the periodic table is an organizational scheme for the elements, what might be some other logical ways in which to group the elements that would provide meaningful chemical information in a periodic table of your own devising?
A chunk of an unidentified element (let’s call it element “X”) is reacted with sulfur to form an ionic compound with the chemical formula X2S. Which of the following elements is the most likely identity of X? a. Mg b. Li c. Al d. C e. Cl
In which of the following are the name and formula correctly paired? a. sodium sulfite: Na2S b. calcium carbonate: Ca(CO3)2 c. magnesium hydroxide: Mg(OH)2 d. nitrite: NO2 e. iron (III) oxide: FeO
The atomic mass of Ga is 69.72 amu. There are only two naturally occurring isotopes of gallium: 69Ga, with a mass of 69.0 amu, and 71Ga, with a mass of 71.0 amu. The natural abundance of the 69Ga isotope is approximately: a. 15% b. 30% c. 50% d. 65% e. 80%
How many protons, neutrons, and electrons are in 119Sn2+? a. 50 p, 69 n, 48 e-b. 50 p, 69 n, 50 e- c. 119 p, 50 n, 69 e- d. 69 p, 50 n, 69 e0 e. 50 p, 119 n, 52 e-
Explain what is meant by the term balanced chemical equation.
Give an example of a binary compound that is ionic. Give an example of a binary compound that is molecular.
Ethane consists of molecules with two atoms of carbon and six atoms of hydrogen. Write the molecular formula for ethane.
Cite some properties that are characteristic of a metal.
What is the name of the element in Group IVA and Period 5?
Oxygen consists of three different __________, each having eight protons but different numbers of neutrons.
What do the various chromatographic separation techniques have in common?
All good experiments start with a scientific question. What was the scientific question that Art Fry was trying to answer when he embarked on finding the adhesive for the Post-it Note?
What are some characteristics of the adhesive used for Post-it Notes?
Vanadium metal is added to steel to impart strength. The density of vanadium is 5.96 g/cm3. Express this in SI units (kg/m3).
The density of magnesium metal (used in fireworks) is 1.74 g/cm3. Express this density in SI units (kg/m3).

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General Chemistry 9th edition Darrell Ebbing, Steven D. Gammon - Solutions

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