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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

Iodine is made by the following reaction (a) Name the two reactants.(b) If you wish to prepare 1.00 kg of I2, what masses of NaIO3 and NaHSO3 are required?(c) What is the theoretical yield of I2 if
Boron forms a series of compounds with hydrogen, all with the general formula BxHy.If 0.148 g of one of these compounds gives 0.422 g of B2O3 when burned in excess O2, what is its empirical formula?
Saccharin, an artificial sweetener, has the formula C7H5NO3S. Suppose you have a sample of a saccharin-containing sweetener with a mass of 0.2140 g. After decomposition to free the sulfur and convert
Silicon and hydrogen form a series of compounds with the general formula SixHy. To find the formula of one of them, a 6.22-g sample of the compound is burned in oxygen. All of the Si is converted to
Menthol, from oil of mint, has a characteristic odor. The compound contains only C, H, and O. If 95.6 mg of menthol burns completely in O2, and gives 269 mg of CO2 and 111 mg of H2O, what is the
Benzoquinone, a chemical used in the dye industry and in photography, is an organic compound containing only C, H, and O. What is the empirical formula of the compound if 0.105 g of the compound
Aqueous solutions of iron(II) chloride and sodium sulfide react to form iron(II)sulfide and sodium chloride.(a) Write the balanced equation for the reaction.(b) If you combine 40. g each of Na2S and
In an experiment, 1.056 g of a metal carbonate, containing an unknown metal M, is heated to give the metal oxide and 0.376 g CO2.What is the identity of the metal M?(a) M = Ni(b) M = Cu(c) M = Zn(d)
Sulfuric acid can be prepared starting with the sulfide ore, cuprite (Cu2S). If each S atom in Cu2S leads to one molecule of H2SO4, what is the theoretical yield of H2SO4 from 3.00 kg of Cu2S?
An unknown metal reacts with oxygen to give the metal oxide, MO2. Identify the metal if a 0.356-g sample of the metal produces 0.452 g of the metal oxide.
Potassium perchlorate is prepared by the following sequence of reactionsWhat mass of Cl2(g) is required to produce 234 kg of KClO4? Cl₂(g) + 2 KOH(aq) → KCl(aq) + KCIO(aq) + H₂O(l) 3 KCIO(aq)
Commercial sodium “hydrosulfite” is 90.1% Na2S2O4. The sequence of reactions used to prepare the compound is(a) What mass of pure Na2S2O4 can be prepared from 125 kg of Zn, 500. g of SO2, and an
Titanium(IV) oxide, TiO2, is heated in hydrogen gas to give water and a new titanium oxide, TixOy. If 1.598 g of TiO2 produces 1.438 g of TixOy, what is the empirical formula of the new oxide?
What mass of lime, CaO, can be obtained by heating 125 kg of limestone that is 95.0% by mass CaCO3? CaCO3(s)→ CaO(s) + CO₂(g)
The elements silver, molybdenum, and sulfur combine to form Ag2MoS4. What is the maximum mass of Ag2MoS4 that can be obtained if 8.63 g of silver, 3.36 g of molybdenum, and 4.81 g of sulfur are
Cloth can be waterproofed by coating it with a silicone layer. This is done by exposing the cloth to (CH3)2SiCl2 vapor. The silicon compound reacts with OH groups on the cloth to form a waterproofing
A mixture of butene, C4H8, and butane, C4H10, is burned in air to give CO2 and water. Suppose you burn 2.86 g of the mixture and obtain 8.80 g of CO2 and 4.14 g of H2O. What are the mass percentages
Copper metal can be prepared by roasting copper ore, which can contain cuprite (Cu2S) and copper(II) sulfide.Suppose an ore sample contains 11.0% impurity in addition to a mixture of CuS and Cu2S.
An Alka-Seltzer tablet contains exactly 100. mg of citric acid, H3C6H5O7, plus some sodium bicarbonate. What mass of sodium bicarbonate is required to consume 100. mg of citric acid by the following
Sodium bicarbonate and acetic acid react according to the equation What mass of sodium acetate can be obtained from mixing 15.0 g of NaHCO3 with 125 mL of 0.15 M acetic acid? NaHCO3(aq) +
A noncarbonated soft drink contains an unknown amount of citric acid, H3C6H5O7. If 100. mL of the soft drink requires 33.51 mL of 0.0102 M NaOH to neutralize the citric acid completely, what mass of
Sodium thiosulfate, Na2S2O3, is used as a “fixer” in black-and-white photography. Suppose you have a bottle of sodium thiosulfate and want to determine its purity. The thiosulfate ion can be
You have a mixture of oxalic acid, H2C2O4, and another solid that does not react with sodium hydroxide. If 29.58 mL of 0.550 M NaOH is required to titrate the oxalic acid in the 4.554-g sample to the
(a) What is the pH of a 0.105 M HCl solution?(b) What is the hydronium ion concentration in a solution with a pH of 2.56? Is the solution acidic or basic?(c) A solution has a pH of 9.67. What is the
A solution of hydrochloric acid has a volume of 125 mL and a pH of 2.56. What mass of NaHCO3 must be added to completely consume the HCl?
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting
You place 2.56 g of CaCO3 in a beaker containing 250. mL of 0.125 M HCl. When the reaction has ceased, does any calcium carbonate remain? What mass of CaCl2 can be produced? CaCO3(s) + 2 HCl(aq)
The cancer drug cisplatin, Pt(NH3)2Cl2, can be made by reacting (NH4)2PtCl4 with ammonia in aqueous solution. Besides cisplatin, the other product is NH4Cl.(a) Write a balanced equation for this
A solution of hydrochloric acid has a volume of 250. mL and a pH of 1.92. Exactly 250. mL of 0.0105 M NaOH is added. What is the pH of the resulting solution?
Calcium and magnesium carbonates occur together in the mineral dolomite. Suppose you heat a sample of the mineral to obtain the oxides, CaO and MgO, and then treat the oxide sample with hydrochloric
You need to know the volume of water in a small swimming pool, but, owing to the pool’s irregular shape, it is not a simple matter to determine its dimensions and calculate the volume. To solve the
Gold can be dissolved from gold-bearing rock by treating the rock with sodium cyanide in the presence of oxygen.(a) Name the oxidizing and reducing agents in this reaction. What has been oxidized,
One type of reaction used in the chemical industry is a substitution, where one atom or group is exchanged for another. In this reaction, an alcohol, 1-butanol, is transformed into 1-bromobutane by
Ethylene oxide, C2H4O, is an important industrial chemical [as it is the starting place to make such important chemicals as ethylene glycol (antifreeze) and various polymers]. One way to make the
You mix 25.0 mL of 0.234 M FeCl3 with 42.5 mL of 0.453 M NaOH.(a) What mass of Fe(OH)3 (in grams) will precipitate from this reaction mixture?(b) One of the reactants (FeCl3 or NaOH) is present in a
In some laboratory analyses, the preferred technique is to dissolve a sample in an excess of acid or base and then “back-titrate” the unreacted acid or base with a standard base or acid. To
A compound consisting of yttrium(III) ions, barium(II) ions, both copper(II) and copper(III) ions, and oxide ions is a superconducting material at low temperatures. It has the formula
Suppose you dilute 25.0 mL of a 0.110 M solution of Na2CO3 to exactly 100.0 mL. You then take exactly 10.0 mL of this diluted solution and add it to a 250-mL volumetric flask. After filling the
You wish to determine the weight percent of copper in a copper-containing alloy. After dissolving a 0.251-g sample of the alloy in acid, an excess of KI is added, and the Cu2+ and I− ions undergo
Oyster beds in the oceans require chloride ions for growth. The minimum concentration is 8 mg/L (8 parts per million). To analyze for the amount of chloride ion in a 50.0-mL sample of water, you add
A compound has been isolated that can have either of two possible formulas:(a) K[Fe(C2O4)2(H2O)2] or(b) K3[Fe(C2O4)3]. To find which is correct, you dissolve a weighed sample of the compound in acid,
Chromium(III) chloride forms many compounds with ammonia. To find the formula of one of these compounds, you titrate the NH3 in the compound with standardized acid. Assume that 24.26 mL of 1.500 M
Thioridazine, C21H26N2S2, is a pharmaceutical agent used to regulate dopamine. (Dopamine, a neurotransmitter, affects brain processes that control movement, emotional response, and ability to
A herbicide contains 2,4-D (2,4-dichlorophenoxyacetic acid), C8H6Cl2O3. A 1.236-g sample of the herbicide was decomposed to liberate the chlorine as Cl− ion. This was precipitated as AgCl, with a
Sulfuric acid is listed in a catalog with a concentration of 95–98%. A bottle of the acid in the stockroom states that 1.00 L has a mass of 1.84 kg. To determine the concentration of sulfuric acid
A 0.5510-g sample consisting of a mixture of iron and iron(III) oxide was dissolved completely in acid to give a solution containing iron(II) and iron(III) ions. A reducing agent was added to convert
Anhydrous calcium chloride is a good drying agent because it will rapidly pick up water. Suppose you have stored some carefully dried CaCl2 in a desiccator. Unfortunately, someone did not close the
Phosphate in urine can be determined by spectrophotometry. After removing protein from the sample, it is treated with a molybdenum compound to give, ultimately, a deep blue polymolybdate. The
A 4.000-g sample containing KCl and KClO4 was dissolved in sufficient water to give 250.00 mL of solution. A 50.00-mL portion of the solution required 41.00 mL of 0.0750 M AgNO3 in a Mohr titration.
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated
Let us explore a reaction with a limiting reactant. Here, zinc metal is added to a flask containing aqueous HCl, and H2 gas is a product.The three flasks each contain 0.100 mol of HCl. Zinc is added
Antacids are chemical compounds that can give immediate relief from indigestion or heartburn because they contain carbonate or hydroxide ions that neutralize stomach acids. Some common active
Maleic anhydride, C4H2O3, can be produced by the oxidation of benzene (Study Question 141). It can also be produced from the oxidation of butene.(a) What is the % atom economy for the synthesis of
Benzene, C6H6, is a common compound, and it can be oxidized to give maleic anhydride, C4H2O3, which is used in turn to make other important compounds.(a) What is the % atom economy for the synthesis
In most states, a person will receive a “driving while intoxicated” (DWI) ticket if the blood alcohol level (BAL) is 80 mg per deciliter (dL) of blood or higher. Suppose a person is found to have
Define the terms system and surroundings. What does it mean to say that a system and its surroundings are in thermal equilibrium?
Identify whether the following processes are exothermic or endothermic. Is the sign on qsys positive or negative? (a) Combustion of methane(b) Melting of ice(c) Raising the temperature of water from
Identify whether the following processes are exothermic or endothermic. Is the sign on qsys positive or negative? (a) The reaction of Na(s) and Cl2(g)(b) Cooling and condensing gaseous N2 to form
The molar heat capacity of mercury is 28.1 J/mol ∙ K. What is the specific heat capacity of this metal in J/g ∙ K?
The specific heat capacity of benzene (C6H6) is 1.74 J/g ∙ K. What is its molar heat capacity (in J/mol ∙ K)?
The specific heat capacity of copper metal is 0.385 J/g ∙ K. How much energy is required to heat 168 g of copper from −12.2°C to +25.6°C?
How much energy as heat is required to raise the temperature of 50.00 mL of water from 25.52°C to 28.75°C? (Density of water at this temperature = 0.997 g/mL.)
The initial temperature of a 344-g sample of iron is 18.2°C. If the sample absorbs 2.25 kJ of energy as heat, what is its final temperature?
After absorbing 1.850 kJ of energy as heat, the temperature of a 0.500-kg block of copper is 37°C. What was its initial temperature?
A 45.5-g sample of copper at 99.8°C is dropped into a beaker containing 152 g of water at 18.5°C. What is the final temperature when thermal equilibrium is reached?
One beaker contains 156 g of water at 22°C, and a second beaker contains 85.2 g of water at 95°C. The water in the two beakers is mixed. What is the final water temperature?
A 182-g sample of gold at some temperature was added to 22.1 g of water. The initial water temperature was 25.0°C, and the final temperature was 27.5°C. If the specific heat capacity of gold is
When 108 g of water at a temperature of 22.5°C is mixed with 65.1 g of water at an unknown temperature, the final temperature of the resulting mixture is 47.9°C. What was the initial temperature of
A 13.8-g piece of zinc is heated to 98.8°C in boiling water and then dropped into a beaker containing 45.0 g of water at 25.0°C. When the water and metal come to thermal equilibrium, the
A 237-g piece of molybdenum, initially at 100.0°C, is dropped into 244 g of water at 10.0°C. When the system comes to thermal equilibrium, the temperature is 15.3°C. What is the specific heat
How much energy is evolved as heat when 1.0 L of water at 0°C solidifies to ice? (The heat of fusion of water is 333 J/g.)
The energy required to melt 1.00 g of ice at 0°C is 333 J. If one ice cube has a mass of 62.0 g and a tray contains 16 ice cubes, what quantity of energy is required to melt a tray of ice cubes to
How much energy is required to vaporize 125 g of benzene, C6H6, at its boiling point, 80.1°C? (The heat of vaporization of benzene is 30.8 kJ/mol.)
Chloromethane, CH3Cl, arises from microbial fermentation and is found throughout the environment. It is also produced industrially, is used in the manufacture of various chemicals, and has been used
The freezing point of mercury is −38.8°C. What quantity of energy, in joules, is released to the surroundings if 1.00 mL of mercury is cooled from 23.0°C to −38.8°C and then frozen to a solid?
What quantity of energy, in joules, is required to raise the temperature of 454 g of tin from room temperature, 25.0°C, to its melting point, 231.9°C, and then melt the tin at that temperature?
A 25.0-mL sample of benzene at 19.9°C was cooled to its melting point, 5.5°C, and then frozen. How much energy was given off as heat in this process? (The density of benzene is 0.80 g/mL, its
As a gas cools, it is compressed from 2.50 L to 1.25 L under a constant pressure of 1.01 × 105 Pa. Calculate the work (in J) required to compress the gas.
A balloon expands from 0.75 L to 1.20 L as it is heated under a constant pressure of 1.01 × 105 Pa. Calculate the work (in J) done by the balloon on the environment.
A balloon does 324 J of work on the surroundings as it expands under a constant pressure of 7.33 × 104 Pa. What is the change in volume (in L) of the balloon?
As the gas trapped in a cylinder with a movable piston cools, 1.34 kJ of work is done on the gas by the surroundings. If the gas is at a constant pressure of 1.33 × 105 Pa, what is the change of
When 745 J of energy in the form of heat is transferred from the environment to a gas, the expansion of the gas does 312 J of work on the environment. What is the change in internal energy of the gas?
The internal energy of a gas decreases by 1.65 kJ when it transfers 1.87 kJ of energy in the form of heat to the surroundings. (a) Calculate the work done by the gas on the surroundings. (b) Does
A volume of 1.50 L of argon gas is confined in a cylinder with a movable piston under a constant pressure of 1.22 × 105 Pa. When 1.25 kJ of energy in the form of heat is transferred from the
Nitrogen monoxide, a gas recently found to be involved in a wide range of biological processes, reacts with oxygen to give brown NO2 gas.Is this reaction endothermic or exothermic? What is the
Nitrogen gas is confined in a cylinder with a movable piston under a constant pressure of 9.95 × 104 Pa. When 695 J of energy in the form of heat is transferred from the gas to the surroundings, its
Calcium carbide, CaC2, is manufactured by the reaction of CaO with carbon at a high temperature. (Calcium carbide is then used to make acetylene.)Is this reaction endothermic or exothermic? What is
Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give water and carbon dioxide.What is the enthalpy change if you burn 1.00 L of isooctane (d =
Acetic acid, CH3CO2H, is made industrially by the reaction of methanol and carbon monoxide.What is the enthalpy change for producing 1.00 L of acetic acid (d = 1.044 g/mL) by this reaction? CH₂OH()
Assume you mix 100.0 mL of 0.200 M CsOH with 50.0 mL of 0.400 M HCl in a coffee-cup calorimeter. The following reaction occurs: The temperature of both solutions before mixing was 22.50°C, and it
You mix 125 mL of 0.250 M CsOH with 50.0 mL of 0.625 M HF in a coffee-cup calorimeter, and the temperature of both solutions rises from 21.50°C before mixing to 24.40°C after the reaction.What is
Adding 5.44 g of NH4NO3(s) to 150.0 g of water in a coffee-cup calorimeter (with stirring to dissolve the salt) resulted in a decrease in temperature from 18.6°C to 16.2°C. Calculate the enthalpy
A piece of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5°C and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 21.7°C. When thermal equilibrium is
You should use care when dissolving H2SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.2 g of concentrated H2SO4(ℓ) was added (with stirring) to 135 g of
A piece of chromium metal with a mass of 24.26 g is heated in boiling water to 98.3°C and then dropped into a coffee-cup calorimeter containing 82.3 g of water at 23.3°C. When thermal equilibrium
Suppose you burned 0.300 g of C(s) in an excess of O2(g) in a constant-volume calorimeter to give CO2(g).The temperature of the calorimeter, which contained 775 g of water, increased from 25.00°C to
Suppose you burned 1.500 g of benzoic acid, C6H5CO2H, in a constant-volume calorimeter and found that the temperature increased from 22.50°C to 31.69°C. The calorimeter contained 775 g of water,
The enthalpy changes for the following reactions can be measured: (a) Use these values and Hess’s law to determine the enthalpy change for the reaction(b) Draw an energy level diagram that shows
A 0.692-g sample of glucose, C6H12O6, was burned in a constant-volume calorimeter. The temperature rose from 21.70°C to 25.22°C. The calorimeter contained 575 g of water, and the bomb had a heat
The enthalpy changes of the following reactions can be measured:(a) Use these values and Hess’s law to determine the enthalpy change for the reaction(b) Draw an energy level diagram that shows the

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