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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

The standard enthalpy of formation of solid barium oxide, BaO, is −553.5 kJ/mol, and the standard enthalpy of formation of barium peroxide, BaO2, is −634.3 kJ/mol.(a) Calculate the standard
An important step in the production of sulfuric acid is the oxidation of SO2 to SO3.Formation of SO3 from the air pollutant SO2 is also a key step in the formation of acid rain.(a) Use standard
The enthalpy change for the oxidation of naphthalene, C10H8, is measured by calorimetry.Use this value, along with the standard enthalpies of formation of CO2(g) and H2O(ℓ), to calculate the
The enthalpy change for the oxidation of styrene, C8H8, is measured by calorimetry.Use this value, along with the standard enthalpies of formation of CO2(g) and H2O(ℓ), to calculate the enthalpy of
The following terms are used extensively in thermodynamics. Define each and give an example.(a) Exothermic and endothermic(b) System and surroundings(c) Specific heat capacity(d) State function(e)
For each of the following, tell whether the process is exothermic or endothermic. (a) H₂O(l) → H₂O(s) (b) 2 H₂(g) + O₂(g) → 2 H₂O(g) (c) H₂O(l, 25 °C) → H₂O(ł, 15 °C) (d)
For each of the following, define a system and its surroundings, and give the direction of energy transfer between system and surroundings.(a) Methane burns in a gas furnace in your home.(b) Water
You have a large balloon containing 1.0 mol of gaseous water vapor at 80°C. How will each step affect the internal energy of the system?(a) The temperature of the system is raised to 90°C.(b) The
Determine whether energy as heat is evolved or required, and whether work was done on the system or whether the system does work on the surroundings, in the following processes at constant
Determine whether energy as heat is evolved or required, and whether work was done on the system or whether the system does work on the surroundings, in the following processes at constant
Use standard enthalpies of formation to calculate the enthalpy change that occurs when 1.00 g of SnCl4(ℓ) reacts with excess H2O(ℓ) to form SnO2(s) and HCl(aq).
You add 100.0 g of water at 60.0°C to 100.0 g of ice at 0.00°C. Some of the ice melts and cools the water to 0.00°C. When the ice and water mixture reaches thermal equilibrium at 0°C, how much
Calculate the quantity of energy required to convert 60.1 g of H2O(s) at 0.0°C to H2O(g) at 100.0°C. The enthalpy of fusion of ice at 0°C is 333 J/g; the enthalpy of vaporization of liquid water
Chloromethane, CH3Cl, a compound found throughout the environment, is formed in the reaction of chlorine atoms with methane.(a) Calculate the enthalpy change for the reaction of CH4(g) and Cl atoms
Insoluble AgCl(s) precipitates when solutions of AgNO3(aq) and NaCl(aq) are mixed.To measure the energy evolved in this reaction, 250. mL of 0.16 M AgNO3(aq) and 125 mL of 0.32 M NaCl(aq) are mixed
Insoluble PbBr2(s) precipitates when solutions of Pb(NO3)2(aq) and NaBr(aq) are mixed.To measure the enthalpy change, 200. mL of 0.75 M Pb(NO3)2(aq) and 200. mL of 1.5 M NaBr(aq) are mixed in a
On a cold day, you can warm your hands with a “heat pad,” a device that uses the oxidation of iron to produce energy as heat.What mass of iron is needed to supply the energy required to warm 15
The reaction of iron(III) oxide with aluminum to give molten iron is known as the thermite reaction.What amount of Al, in moles, is needed for complete reaction with 3.0 mol of Fe2O3? What mass of
What mass of HCl, in grams, is required to react with 0.750 g of Al(OH)3? What mass of water, in grams, is produced? Al(OH)3(s) + 3 HCl(aq) → AlCl3(aq) + 3 H₂O(l)
Like many metals, aluminum reacts with a halogen (here the orange-brown liquid Br2) to give a metal halide, aluminum bromide. (The white solid on the lip of the beaker at the end of the reaction is
The balanced equation for the reduction of iron ore to the metal using CO is(a) What is the maximum mass of iron, in grams, that can be obtained from 454 g (1.00 lb) of iron(III) oxide?(b) What mass
The formation of water-insoluble silver chloride is useful in the analysis of chloride-containing substances. Consider the following unbalanced equation: (a) Write the balanced equation.(b) What
Methane, CH4, burns in oxygen.(a) What are the products of the reaction?(b) Write the balanced equation for the reaction.(c) What mass of O2, in grams, is required for complete combustion of 25.5 g
The metals industry was a major source of air pollution years ago. One common process involved “roasting” metal sulfides in the air:If 2.50 mol of PbS is heated in air, what amount of O2 is
Iron ore is converted to iron metal in a reaction with carbon.If 6.2 mol of Fe2O3(s) is used, what amount of C(s) is needed, and what amounts of Fe and CO2 are produced? 2 Fe₂O3(s) + 3 C(s)→ 4
Chromium metal reacts with oxygen to give chromium(III) oxide, Cr2O3.(a) Write a balanced equation for the reaction.(b) What mass (in grams) of Cr2O3 is produced if 0.175 g of chromium metal is
Sodium sulfide, Na2S, is used in the leather industry to remove hair from hides. The Na2S is made by the reactionSuppose you mix 15 g of Na2SO4 and 7.5 g of C. Which is the limiting reactant? What
Ethane, C2H6, burns in oxygen.(a) What are the products of the reaction?(b) Write the balanced equation for the reaction.(c) What mass of O2, in grams, is required for complete combustion of 13.6 of
Ammonia gas can be prepared by the reaction of a metal oxide such as calcium oxide with ammonium chloride.If 112 g of CaO and 224 g of NH4Cl are mixed, what is the limiting reactant, and what mass of
The compound SF6 is made by burning sulfur in an atmosphere of fluorine. The balanced equation is Starting with a mixture of 1.6 mol of sulfur, S8, and 35 mol of F2,(a) Which is the limiting
Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine:Starting with a mixture of 32.0 g of sulfur and 71.0 g of Cl2,(a) Which is the
The reaction of methane and water is one way to prepare hydrogen for use as a fuel: If you begin with 995 g of CH4 and 2510 g of water, (a) Which reactant is the limiting reactant?(b) What is the
Aluminum chloride, AlCl3, is made by treating scrap aluminum with chlorine.If you begin with 2.70 g of Al and 4.05 g of Cl2,(a) Which reactant is limiting?(b) What mass of AlCl3 can be produced?(c)
In the thermite reaction, iron(III) oxide is reduced by aluminum to give molten iron. If you begin with 10.0 g of Fe2O3 and 20.0 g of Al,(a) Which reactant is limiting?(b) What mass of Fe can be
In Example 4.2, you found that a particular mixture of CO and H2 could produce 407 g CH3OH.If only 332 g of CH3OH is actually produced, what is the percent yield of the compound?Data given in Example
Aspirin, C6H4(OCOCH3)CO2H, is produced by the reaction of salicylic acid, C6H4(OH)CO2H, and acetic anhydride, (CH3CO)2O .If you mix 100. g of each of the reactants, what is the maximum mass of
Ammonia gas can be prepared by the following reaction: If 112 g of CaO and 224 g of NH4Cl are mixed, the theoretical yield of NH3 is 68.0 g. If only 16.3 g of NH3 is actually obtained, what is its
The deep blue compound Cu(NH3)4SO4 is made by the reaction of copper(II) sulfate and ammonia. (a) If you use 10.0 g of CuSO4 and excess NH3, what is the theoretical yield of Cu(NH3)4SO4?(b) If you
Black smokers are found in the depths of the oceans. Thinking that the conditions in these smokers might be conducive to the formation of organic compounds, two chemists in Germany found the
The reaction of methane and water is one way to prepare hydrogen for use as a fuel:If this reaction has a 37% yield under certain conditions, what mass of CH4 is required to produce 15 g of H2?
Methanol, CH3OH, can be prepared from carbon monoxide and hydrogen.What mass of hydrogen is required to produce 1.0 L of CH3OH (d = 0.791 g/mL) if this reaction has a 74% yield under certain
A mixture of CuSO4 and CuSO4 ⋅ 5 H2O has a mass of 1.245 g. After heating to drive off all the water, the mass is only 0.832 g. What is the mass percent of CuSO4 ⋅ 5 H2O in the mixture?
A sample of limestone and other soil materials was heated, and the limestone decomposed to give calcium oxide and carbon dioxide. A 1.506-g sample of limestone-containing material gave 0.558 g of
A 2.634-g sample containing impure CuCl2 ⋅ 2 H2O was heated. The sample mass after heating to drive off the water was 2.125 g. What was the mass percent of CuCl2 ⋅ 2 H2O in the original sample?
Nickel(II) sulfide, NiS, occurs naturally as the relatively rare mineral millerite. One of its occurrences is in meteorites. To analyze a mineral sample for the quantity of NiS, the sample is
At higher temperatures, NaHCO3 is converted quantitatively to Na2CO3.Heating a 1.7184-g sample of impure NaHCO3 gives 0.196 g of CO2. What was the mass percent of NaHCO3 in the original 1.7184-g
The aluminum in a 0.764-g sample of an unknown material was precipitated as aluminum hydroxide, Al(OH)3, which was then converted to Al2O3 by heating strongly. If 0.127 g of Al2O3 is obtained from
Styrene, the building block of polystyrene, consists of only C and H. If 0.438 g of styrene is burned in oxygen and produces 1.481 g of CO2 and 0.303 g of H2O, what is the empirical formula of
Mesitylene is a liquid hydrocarbon. Burning 0.115 g of the compound in oxygen gives 0.379 g of CO2 and 0.1035 g of H2O. What is the empirical formula of mesitylene?
Naphthalene is a hydrocarbon that once was used in mothballs. If 0.3093 g of the compound is burned in oxygen, 1.0620 g of CO2 and 0.1739 g of H2O are isolated. (a) What is the empirical formula of
Azulene is a beautiful blue hydrocarbon. If 0.106 g of the compound is burned in oxygen, 0.364 g of CO2 and 0.0596 g of H2O are isolated. (a) What is the empirical formula of azulene?(b) If a
An unknown compound has the formula CxHyOz. You burn 0.0956 g of the compound and isolate 0.1356 g of CO2 and 0.0833 g of H2O. What is the empirical formula of the compound? If the molar mass is 62.1
An unknown compound has the formula CxHyOz. You burn 0.1523 g of the compound and isolate 0.3718 g of CO2 and 0.1522 g of H2O. What is the empirical formula of the compound? If the molar mass is 72.1
Nickel forms a compound with carbon monoxide, Nix(CO)y. To determine its formula, you carefully heat a 0.0973-g sample in air to convert the nickel to 0.0426 g of NiO and the CO to 0.100 g of CO2.
To find the formula of a compound composed of iron and carbon monoxide, Fex(CO)y, the compound is burned in pure oxygen to give Fe2OTo find the formula of a compound composed3 and CO2. If you burn
If 6.73 g of Na2CO3 is dissolved in enough water to make 250. mL of solution, what is the molar concentration of the sodium carbonate? What are the molar concentrations of the Na+ and CO32− ions?
Some potassium dichromate (K2Cr2O7), 2.335 g, is dissolved in enough water to make exactly 500. mL of solution. What is the molar concentration of the potassium dichromate? What are the molar
What is the mass of solute, in grams, in 250. mL of a 0.0125 M solution of KMnO4?
What is the mass of solute, in grams, in 125 mL of a 1.023 × 10−3 M solution of Na3PO4? What is the molar concentration of the Na+ and PO43− ion?
What volume of 0.123 M NaOH, in milliliters, contains 25.0 g of NaOH?
What volume of 2.06 M KMnO4, in liters, contains 322 g of solute?
Identify the ions that exist in each aqueous solution, and specify the concentration of each ion.(a) 0.25 M (NH4)2SO4(b) 0.123 M Na2CO3(c) 0.056 M HNO3
Identify the ions that exist in each aqueous solution, and specify the concentration of each ion.(a) 0.12 M BaCl2(b) 0.0125 M CuSO4(c) 0.500 M K2Cr2O7
An experiment in your laboratory requires 500. mL of a 0.0200 M solution of Na2CO3. You are given solid Na2CO3, distilled water, and a 500.-mL volumetric flask. Describe how to prepare the required
What mass of oxalic acid, H2C2O4, is required to prepare 250. mL of a solution that has a concentration of 0.15 M H2C2O4
If you dilute 25.0 mL of 1.50 M hydrochloric acid to 500. mL, what is the molar concentration of the dilute acid?
If 4.00 mL of 0.0250 M CuSO4 is diluted to 10.0 mL with pure water, what is the molar concentration of copper(II) sulfate in the diluted solution?
Which of the following methods would you use to prepare 1.00 L of 0.125 M H2SO4?(a) Dilute 20.8 mL of 6.00 M H2SO4 to a volume of 1.00 L.(b) Add 950. mL of water to 50.0 mL of 3.00 M H2SO4.
Which of the following methods would you use to prepare 300. mL of 0.500 M K2Cr2O7?(a) Add 30.0 mL of 1.50 M K2Cr2O7 to 270. mL of water.(b) Dilute 250. mL of 0.600 M K2Cr2O7 to a volume of 300. mL.
You have 250. mL of 0.136 M HCl. Using a volumetric pipet, you take 25.00 mL of that solution and dilute it to 100.00 mL in a volumetric flask. Now you take 10.00 mL of that solution, using a
Suppose you have 100.00 mL of a solution of a dye and transfer 2.00 mL of the solution to a 100.00-mL volumetric flask. After adding water to the 100.00 mL mark, you take 5.00 mL of that solution and
A saturated solution of milk of magnesia, Mg(OH)2, has a pH of 10.5. What is the hydronium ion concentration of the solution? Is the solution acidic or basic?
What is the hydronium ion concentration of a 0.0013 M solution of HNO3? What is its pH?
Make the following conversions. In each case, tell whether the solution is acidic or basic. (a) (b) (c) (d) pH 1.00 10.50 [H3O+] 1.3 x 10-5 M 2.3 × 10-8 M
What is the hydronium ion concentration of a 1.2 × 10−4 M solution of HClO4? What is its pH?
What volume of 0.109 M HNO3, in milliliters, is required to react completely with 2.50 g of Ba(OH)2? 2 HNO3(aq) + Ba(OH)₂(s) - 2 H₂O(l) + Ba(NO3)2(aq)
What mass of Na2CO3, in grams, is required for complete reaction with 50.0 mL of 0.125 M HNO3? Na₂CO3(aq) + 2 HNO3(aq) — 2 NaNO3(aq) + CO₂(g) + H₂O(l)
When an electric current is passed through an aqueous solution of NaCl, the valuable industrial chemicals H2(g), Cl2(g), and NaOH are produced. What mass of NaOH can be formed from 15.0 L of 0.35 M
Hydrazine, N2H4, a base like ammonia, can react with sulfuric acid.What mass of hydrazine reacts with 250. mL of 0.146 M H2SO4? 2 N₂H₂(aq) + H₂SO4(aq) → 2 N₂H5+ (aq) + SO4²- (aq)
In the photographic developing process, silver bromide is dissolved by adding sodium thiosulfate. If you want to dissolve 0.225 g of AgBr, what volume of 0.0138 M Na2S2O3, in milliliters, should be
You can dissolve an aluminum soft drink can in an aqueous base such as potassium hydroxide.If you place 2.05 g of aluminum in a beaker with 185 mL of 1.35 M KOH, will any aluminum remain? What mass
What volume of 0.750 M Pb(NO3)2, in milliliters, is required to react completely with 1.00 L of 2.25 M NaCl solution? The balanced equation is Pb(NO3)2(aq) + 2 NaCl(aq) → PbCl₂(s) + 2 NaNO3(aq)
What volume of 0.125 M oxalic acid, H2C2O4, is required to react with 35.2 mL of 0.546 M NaOH? H₂C₂O4(aq) + 2 NaOH(aq) Na₂C₂O4(aq) + 2 H₂O(l)
What volume of 0.812 M HCl, in milliliters, is required to titrate 1.45 g of NaOH to the equivalence point? NaOH(aq) + HCl(aq) → H₂O(l) + NaCl(aq)
What volume of 0.955 M HCl, in milliliters, is required to titrate 2.152 g of Na2CO3 to the equivalence point? Na₂CO3(aq) + 2 HCl(aq) – H₂O(l) + CO₂(g) + 2 NaCl(aq)
If 38.55 mL of HCl is required to titrate 2.150 g of Na2CO3 according to the following equation, what is the concentration (mol/L) of the HCl solution? Na₂CO3(aq) + 2 HCl(aq) - 2 NaCl(aq) +
Potassium hydrogen phthalate, KHC8H4O4, is used to standardize solutions of bases. The acidic anion reacts with strong bases according to the following net ionic equation:If a 0.902-g sample of
You have 0.954 g of an unknown acid, H2A, which reacts with NaOH according to the balanced equationIf 36.04 mL of 0.509 M NaOH is required to titrate the acid to the second equivalence point, what is
An unknown solid acid is either citric acid or tartaric acid. To determine which acid you have, you titrate a sample of the solid with aqueous NaOH and from this determine the molar mass of the
To analyze an iron-containing compound, you convert all the iron to Fe2+ in aqueous solution and then titrate the solution with standardized KMnO4. The balanced, net ionic equation isA 0.598-g sample
Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an
A solution of a dye was analyzed by spectrophotometry, and the following calibration data were collected.(a) Construct a calibration plot, and determine the slope and intercept.(b) What is the dye
The nitrite ion is involved in the biochemical nitrogen cycle. You can determine the nitrite ion content of a sample using spectrophotometry by first using several organic compounds to form a colored
The metabolic disorder diabetes causes a buildup of acetone, CH3COCH3, in the blood. Acetone, a volatile compound, is exhaled, giving the breath of untreated diabetics a distinctive odor. The acetone
Suppose 16.04 g of benzene, C6H6, is burned in oxygen. (a) What are the products of the reaction?(b) Write a balanced equation for the reaction.(c) What mass of O2, in grams, is required for
Your body deals with excess nitrogen by excreting it in the form of urea, NH2CONH2. The reaction producing it is the combination of arginine (C6H14N4O2) with water to give urea and ornithine
The reaction of iron metal and chlorine gas to give iron(III) chloride is illustrated below. (a) Write the balanced chemical equation for the reaction.(b) Beginning with 10.0 g of iron, what mass of
Some metal halides react with water to produce the metal oxide and the appropriate hydrogen halide (see photo). For example,(a) Name the four compounds involved in this reaction.(b) If you begin with
The reaction of 750. g each of NH3 and O2 was found to produce 562 g of NO.(a) What mass of water is produced by this reaction?(b) What mass of O2 is required to consume 750. g of NH3? 4 NH3(g) + 5
Sodium azide, an explosive chemical used in automobile airbags, is made by the following reaction:If you combine 15.0 g of NaNO3 with 15.0 g of NaNH2, what mass of NaN3 is produced? NaNO3 + 3 NaNH,

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