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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

Galvanized steel pipes are used in the plumbing of many older homes. When copper plumbing is added to a system consisting of galvanized steel pipes it is necessary to place an insulator between the
Consider an electrochemical cell based on the half-reactions Ni2+(aq) + 2 e− → Ni(s) and Cd2+(aq) +2 e− → Cd(s).(a) Diagram the cell, and label each of the components (including the anode,
An old method of measuring the current flowing in a circuit was to use a “silver coulometer.” The current passed first through a solution of Ag+(aq) and then into another solution containing an
A “silver coulometer” (Study Question 106) was used in the past to measure the current flowing in an electrochemical cell. Suppose you found that the current flowing through an electrolysis cell
Four metals, A, B, C, and D, exhibit the following properties:(a) Only A and C react with l.0 M hydrochloric acid to give H2(g).(b) When C is added to solutions of the ions of the other metals,
A solution of KI is added dropwise to a pale blue solution of Cu(NO3)2. The solution changes to a brown color, and a precipitate of CuI forms. In contrast, no change is observed if solutions of KCl
Fluorinated organic compounds are used as herbicides, flame retardants, and fire-extinguishing agents, among other things. A reaction such asis carried out electrochemically in liquid HF as the
The amount of oxygen, O2, dissolved in a water sample at 25°C can be determined by titration. The first step is to add solutions of MnSO4 and NaOH to the water to convert the dissolved oxygen to
The free energy change for a reaction, ΔrG°, is the maximum energy that can be extracted from the process as work, whereas ΔrH° is the total chemical potential energy change. The efficiency of a
(a) Is it easier to reduce water in acid or base? To evaluate this, consider the half-reaction(b) What is the reduction potential for water for solutions at pH = 7 (neutral) and pH = 1 (acid)?
A hydrogen-oxygen fuel cell operates on the simple reactionH2(g) + 1/2 O2(g) → H2O(ℓ)If the cell is designed to produce 1.5 A of current and if the hydrogen is contained in a 1.0-L tank at 200
In the discussion on the composition of air, mention is made of the fact that water vapor may have a concentration as high as 40,000 ppm. Calculate the partial pressure exerted by water vapor at this
Which of the following atmospheric gases is present in highest concentration in dry air?(a) N2O(b) CH4(c) O3(d) CO
Many chemical reactions that occur in the atmosphere and stratosphere involve free radicals. Free radical formation occurs when a photon of light is absorbed and the energy of the radiation being
A 2011 article in Science magazine stated that “Public discussion of climate change . . . is just beginning to reflect an awareness of the important role played by the global nitrogen cycle.”
Assume the average CO2 concentration in the atmosphere is 406 ppm (as of January 2017). The actual concentration of CO2 at different sites will vary. Speculate on whether the concentration of CO2
Suppose you find the CO concentration in your home is 10. ppm by volume at 1.00 atm pressure and 25°C. What is the concentration in mg/L and in ppm by mass. (The average molar mass for dry air is
The carbon content in seawater is 30 mmol/L (Table 20.2). This includes both HCO3− and CO32− ions. Knowing the pH of seawater is 8.1, what is the ratio of concentrations of these two ions in
Various reagents are added to water supplies to kill pathogens and make the water safe to drink. Among the substances listed below, which does not serve that function?(a) Cl2(b) O3(c) Ca(ClO)2(d)
Which of the following statements is not correct?(a) Phosphates enhance the growth of algae in surface water.(b) Melting of the polar ice cap will result in a rise in sea levels.(c) Heavy metal
Using the data in Table 20.2, estimate the minimum mass of solid that would remain after evaporation of 1.0 L of seawater.Data given in Table 20.2 Concentrations of Some Cations and Anions TABLE 20.2
In any solution, there must be a balance between the positive and negative charges of the ions that are present. Use the data in Table 20.2 to determine how close to a balance of charge is achieved
What mass of NaCl could be obtained by evaporating 1.0 L of seawater? The amount of Na+ ions in seawater limits the amount of NaCl that can be obtained.
Although there are a number of magnesium-containing minerals, the commercial source of this metal is seawater. Treatment of seawater with Ca(OH)2 gives insoluble Mg(OH)2. This reacts with HCl to
A 2010 article in Science magazine described “Sewage Treatment with Anammox.” [B. Kartal, J. G. Kuenen, and M. C. M. van Loosdrecht, Science, Vol. 328, pp. 702-703, 2010.] The authors noted that
Calculate the mass of Mg that could be obtained by the process described in Study Question 13 from 1.0 L of seawater. To prepare 100. kg of Mg, what volume of seawater would be needed? (The density
Silver ions have long been known to have biocidal properties. The increasing use of silver for this purpose has led to greater silver concentrations in waste water, and there has been some concern
Which of the following is a renewable energy resource?(a) Nuclear fusion(b) Hydroelectric power(c) Natural gas(d) Coal
In the United States (and worldwide), fossil fuels provide the larger source of energy. What is the second largest energy source?(a) Hydroelectric(b) Solar(c) Nuclear(d) Geothermal
Use the value for “energy released” in kilojoules per gram from gasoline listed in Table 20.4 to estimate the percentage of carbon, by mass, in gasoline.Data given in Table 20.4 TABLE 20.4 Energy
Hydrogen can be produced using the reaction of steam (H2O) with various hydrocarbons. Compare the mass of H2 expected from the reaction of steam with 100. g each of methane, petroleum, and coal.
The enthalpy of combustion of isooctane (C8H18), one of the many hydrocarbons in gasoline, is 5.45 × 103 kJ/mol. Calculate the enthalpy change per gram of isooctane and per liter of isooctane (d =
Per capita energy consumption in the United States has been equated to the energy obtained by burning 70. lb of coal per day. Use enthalpy of formation data to calculate the energy transferred as
Energy consumption in the United States amounts to the equivalent of the energy obtained by burning 7.0 gal of oil or 70. lb of coal per day per person. Using data in Table 20.4, carry out
Calculate the energy used, in kilojoules, to power a 100‑watt lightbulb continuously over a 24-hour period. How much coal would have to be burned to provide this quantity of energy, assuming that
List the following substances in order of energy released by combustion per gram: C8H18, H2, C(s), CH4. (See Study Question 22 for the enthalpy of combustion of isooctane, C8H18.) Which is the best
Confirm the statement in the text that oxidation of 1.0 L of methanol to form CO2(g) and H2O(ℓ) in a fuel cell will provide at least 5.0 kW-h of energy. (The density of liquid methanol is 0.787
A parking lot in Los Angeles receives an average of 2.6 × 107 J/m2 of solar energy per day in the summer.(a) If the parking lot is 325 m long and 50.0 m wide, what is the total quantity of energy
Your home loses energy in the winter through doors, windows, and any poorly insulated walls. A sliding glass door (6 ft × 6.5 ft with 0.5 inch of insulating glass) allows 1.0 × 106 J/h to pass
Some fuel-efficient hybrid cars are rated at 55.0 miles per gallon of gasoline. Calculate the energy used to drive 1.00 mile if gasoline produces 48.0 kJ/g and the density of gasoline is 0.737 g/cm3.
In methane hydrate the methane molecule is trapped in a cage of water molecules. Describe the structure:(a) How many water molecules make up the cage,(b) How many hydrogen bonds are involved, and(c)
Microwave ovens are highly efficient, compared to other cooking appliances. A 1100-watt microwave oven, running at full power for 90 seconds, will raise the temperature of 1 cup of water (225 mL)
One cubic meter of methane hydrate has 164 m3 of CH4 (at STP). If you burn the methane in 1.00 m3 of hydrate [to give CO2(g) and H2O(g)], how much energy, as heat, can be obtained?
Which of the following is not a limitation for the use of hydrogen as a fuel?(a) An inexpensive method of producing hydrogen(b) A practical means of storing hydrogen(c) Hydrogen is explosive(d) A
Which of the following statements is true?(a) Fuel cells are widely used in automobiles.(b) H2 is readily available as a transportation fuel.(c) Petroleum is a mixture of hydrocarbons.(d) Methane
Methyl myristate, C13H27CO2CH3(ℓ), can be used as a biofuel.(a) Write a balanced chemical equation for the reaction that occurs when 1 mol of methyl myristate, C13H27CO2CH3(ℓ), is burned, forming
Generating hydrogen gas using the least amount of energy possible is very desirable. One proposed scheme is the catalyzed decomposition of formic acid, HCO2H. [S. Ott, Science, Vol. 333, pp.
You want to use electrolysis to plate a cylindrical object (radius = 2.50 and length = 20.00 cm) with a coating of nickel metal, 4.0 mm thick. You place the object in a bath containing a salt
Which of the species listed below is not a greenhouse gas?(a) H2O(b) CH4(c) CO2(d) O2
What is the correlation between ocean pH and atmospheric CO2?(a) As CO2 increases, the pH decreases.(b) As CO2 increases, the pH also increases.(c) As CO2 increases, the pH does not change.
Define the terms renewable and nonrenewable as applied to energy resources. Which of the following energy resources are renewable: solar energy, coal, natural gas, geothermal energy, wind power?
What are the three most abundant gases in the atmosphere? Are any of these greenhouse gases?
What are the environmental consequences of ozone in the troposphere? In the stratosphere?
Compare the advantages and disadvantages of the different methods used to disinfect drinking water.
Mercury, lead, and arsenic in the environment are major concerns. Identify the main source or sources of these pollutants.
What is the likelihood that hydrogen (H2) will become a widely used fuel and that the “hydrogen economy” will become a reality? In particular, what are the advantages and disadvantages of H2 as a
Refer to Figure 20.6. What is the average rate of increase in atmospheric CO2 per year? Assuming the rate of increase continues at the same pace, predict the approximate concentration of CO2 in the
An understanding of most environmental issues requires one to consider a range of factors— economic, political, sociological, as well as scientific. Bearing this in mind, discuss each of the issues
Which sulfur compounds are atmospheric pollutants? What is their origin? Describe steps being taken to prevent sulfur compounds from entering the atmosphere.
Which of the following formulas is incorrect?(a) CaH2(b) CaI2(c) CaS(d) Ca2O3
The reaction of elemental phosphorus and excess oxygen produces P4O10. Name the compound.(a) Phosphorus oxide(b) Phosphoric acid(c) Phosphorus decaoxide(d) Tetraphosphorus decaoxide
Like sulfur, selenium forms compounds in several different oxidation states. Which of the following is NOT likely to be an oxidation state of selenium in its compounds?(a) −2(b) +3(c) +6 (d) +4
What is the highest oxidation state that antimony can have in its compounds?(a) 0 (b) +1 (c) +3 (d) +5
Give examples of two basic oxides. Write equations illustrating the formation of each oxide from its component elements. Write another chemical equation that illustrates the basic character of each
Give examples of two acidic oxides. Write equations illustrating the formation of each oxide from its component elements. Write another chemical equation that illustrates the acidic character of each
Give the name and symbol of each element having the valence configuration [noble gas] ns2np1.
Give symbols and names for four monatomic ions that have the same electron configuration as argon.
Select one of the alkali metals, and write a balanced chemical equation for its reaction with chlorine. Is the reaction likely to be exothermic or endothermic? Is the product ionic or molecular?
Select one of the alkaline earth metals and write a balanced chemical equation for its reaction with oxygen. Is the reaction likely to be exothermic or endothermic? Is the product ionic or molecular?
For the product of the reaction you selected in Study Question 9, predict the following physical properties: color, state of matter (s, ℓ, or g), solubility in water.Data given in Question 9Select
For the product of the reaction you selected in Study Question 10, predict the following physical properties: color, state of matter (s, ℓ, or g), solubility in water.Data given in Question
Would you expect to find calcium occurring naturally in the Earth’s crust as a free element? Why or why not?
Which of the first 10 elements in the periodic table are found as free elements in the Earth’s crust? Which elements in this group occur in the Earth’s crust only as part of a chemical compound?
Place the following oxides in order of increasing basicity: CO2, SiO2, SnO2.
Place the following oxides in order of increasing basicity: Na2O, Al2O3, SiO2, SO3.
Complete and balance the equations for the following reactions. [Assume an excess of oxygen for (d).](a) Na(s) + Br2(ℓ) →(b) Mg(s) + O2(g) →(c) Al(s) + F2(g) →(d) C(s) + O2(g) →
Complete and balance the equations for the following reactions:(a) K(s) + I2(g) →(b) Ba(s) + O2(g) →(c) Al(s) + S8(s) →(d) Si(s) + Cl2(g) →
Which of the following elements does not react with hydrogen?(a) Neon(b) Nitrogen(c) Potassium(d) Fluorine
Which of the methods below is the most suitable for the preparation of large quantities of hydrogen (such as the amounts needed as a reagent for the synthesis of compounds such as ammonia)?(a)
Write balanced chemical equations for the reaction of hydrogen gas with oxygen, chlorine, and nitrogen.
Write a balanced chemical equation for the preparation of H2 (and CO) by the reaction of CH4 and water. Using data in Appendix L, calculate ΔrH°, ΔrG°, and ΔrS° for this reaction at 298 K.Data
Write an equation for the reaction of potassium and hydrogen. Name the product. Is it ionic or covalent? Predict one physical property and one chemical property of this compound.
Using data in Appendix L, calculate ΔrH°, ΔrG°, and ΔrS° for the reaction of carbon and water to give CO and H2 at 298 K.Data given in Appendix L TABLE 20 Species Aluminum Al(s) AICI
A method recently suggested for the preparation of hydrogen (and oxygen) from water proceeds as follows:(a) Sulfuric acid and hydrogen iodide are formed from sulfur dioxide, water, and iodine.(b) The
Compare the mass of H2 expected from the reaction of steam (H2O) per mole of methane, petroleum, and coal. (Assume complete reaction in each case. Use CH2 and CH as representative formulas for
Which of the following is not a property of sodium?(a) Reacts with Cl2 to form NaCl(b) Has a high melting point (>400°C)(c) Has a silvery color(d) Conducts an electric current
The compound Na2O2 consists of(a) Two Na+ ions and two O2− ions(b) Molecules of Na2O2(c) Two Na+ ions and one O22− ion(d) Na2+ and O2− ions
Write equations for the reaction of sodium with each of the halogens. Predict at least two physical properties that are common to all of the alkali metal halides.
Write balanced equations for the reaction of lithium, sodium, and potassium with O2. Specify which metal forms an oxide, which forms a peroxide, and which forms a superoxide.
The electrolysis of aqueous NaCl gives NaOH, Cl2, and H2.(a) Write a balanced equation for the process.(b) In the United States, 1.19 × 1010 kg of NaOH and 1.14 × 1010 kg of Cl2 were produced in a
(a) Write equations for the half-reactions that occur at the cathode and the anode when an aqueous solution of KCl is electrolyzed. Which chemical species is oxidized, and which chemical species is
Which of the following insoluble calcium compounds does not dissolve in hydrochloric acid?(a) Limestone, CaCO3(b) Slaked lime, Ca(OH)2(c) Gypsum, CaSO4 ∙ 2 H2O(d) Hydroxyapatite, Ca5(OH)(PO4)3
Calcium minerals are the raw materials for a variety of large-scale industrial processes. Which of the following is not an industrial process?(a) Converting limestone, CaCO3, to lime(b) Converting
Calcium reacts with hydrogen gas at 300−400°C to form a hydride. This compound reacts readily with water, so it is an excellent drying agent for organic solvents.(a) Write a balanced equation
When magnesium burns in air, it forms both an oxide and a nitride. Write balanced equations for the formation of both compounds.
Name three uses of limestone. Write a balanced equation for the reaction of limestone with CO2 in water.
Explain what is meant by “hard water.” What causes hard water, and what problems are associated with it?
Calcium oxide, CaO, is used to remove SO2 from power plant exhaust. These two compounds react to give solid CaSO3. What mass of SO2 can be removed using 1.2 × 103 kg of CaO?
Ca(OH)2 has a Ksp of 5.5 × 10−5, whereas Ksp for Mg(OH)2 is 5.6 × 10−12. Calculate the equilibrium constant for the reactionCa(OH)2(s) + Mg2+(aq) ⇄ Ca2+(aq) + Mg(OH)2(s)Explain why this
In terms of abundance of the elements in the Earth’s crust, aluminum ranks(a) First(b) Second(c) Third(d) Fourth

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