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General Chemistry Principles And Modern Applications 11th Edition Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette - Solutions

(A) A 15.00 mL sample of 0.450 M K2CrO4 is diluted to 100.00 mL. What is the concentration of the new solution?(B) When left in an open beaker for a period of time, the volume of 275 mL of 0.105 M NaCl is found to decrease to 237 mL because of the evaporation of water. What is the new concentration
Write balanced equations to represent:(a) The decomposition, by heating, of solid ammonium nitrate to produce dinitrogen monoxide gas (laughing gas) and water vapor(b) The reaction of aqueous sodium carbonate with hydrochloric acid to produce water, carbon dioxide gas, and aqueous sodium
A particular analytical chemistry procedure requires 0.0100 M K2CrO4. What volume of 0.250 M K2CrO4 must be diluted with water to prepare 0.2500 L of 0.0100 M K2CrO4?
(A) How many milliliters of 0.250 M K2CrO4 must be added to excess AgNO3(aq) to produce 1.50 g Ag2CrO4?(B) How many milliliters of 0.150 M AgNO3 are required to react completely with 175 mL of 0.0855 M K2CrO4? What mass of Ag2CrO4 is formed?
A 25.00 mL pipetful of 0.250 M K2CrO4 is added to an excess of AgNO3(aq). What mass of Ag2CrO4 will precipitate from the solution? K₂CrO₂(aq) + 2 AgNO3(aq) - Ag2CrO4(s) + 2 KNO3(aq)
(A) If 215 g P4 is allowed to react with 725 g Cl2 in the reaction in Example 4-11, how many grams of PCl3 are formed?(B) If 1.00 kg each of PCl3, Cl2 and P4O10 are allowed to react, how many kilograms of POCl3 will be formed?6 PCl3(l) + 6 Cl2(g) + P4O10(s) → 10 POCl3(l)Example 4-11Phosphorus
Write balanced equations to represent:(a) The reaction of sulfur dioxide gas with oxygen gas to produce sulfur trioxide gas (one of the reactions involved in the industrial preparation of sulfuric acid)(b) The dissolving of limestone (calcium carbonate) in water containing dissolved carbon dioxide
Write a balanced chemical equation for the reaction depicted below. +
Phosphorus trichloride, PCl3 is a commercially important compound used in the manufacture of pesticides, gasoline additives, and a number of other products. A ball-and-stick model of PCl3 is shown below. Liquid PCl3 is made by the direct combination of phosphorus and chlorine.What is the maximum
(A) In Practice Example 4-11A, which reactant is in excess and what mass of that reactant remains after the reaction to produce PCl3?(B) If 12.2 g H2 and 154 g O2 are allowed to react, which gas and what mass of that gas remains after the reaction?2 H2(g) + O2(g) → 2 H2O(l)Practice Ex. 4-11(A)If
Write a balanced chemical equation for the reaction depicted below. + +
What mass of P4 remains following the reaction in Example 4-11? Example 4-11 Phosphorus trichloride, PCl3 is a commercially important compound used in the manufacture of pesticides, gasoline additives, and a number of other products. A ball-and-stick model of PCl3 is shown below. Liquid PCl3 is
Billions of kilograms of urea, CO(NH2)2, are produced annually for use as a fertilizer. A ball-and-stick model of urea is shown here. The reaction used is given below.The typical starting reaction mixture has a 3 : 1 mole ratio of NH3 to CO2. If 47.7 g urea forms per mole of CO2 that reacts, what
A: Formaldehyde, CH2O, can be made from methanol by the following reaction, using a copper catalyst. CH3OH(g) → CH2O(g) + H2(g)If 25.7 g CH2O(g) is produced per mole of methanol that reacts, what are (a) The theoretical yield; (b) The actual yield; and (c) The percent yield?(B) What is the
In an experiment, 0.689 g Cr(s) reacts completely with 0.636 g O2 (g) to form a single solid compound. Write a balanced chemical equation for the reaction.
When heated with sulfuric or phosphoric acid, cyclohexanol, C6H11OH, is converted to cyclohexene, C6H10. Ball-and-stick models of cyclohexanol and cyclohexene are shown here. The balanced chemical equation for the reaction is shown below.If the percent yield is 83%, what mass of cyclohexanol must
(A) If the percent yield for the formation of urea in Example 4-13 were 87.5%, what mass of CO2, together with an excess of NH3 would have to be used to obtain 50.0 g CO(NH2)2?(B) Calculate the mass of cyclohexanol (C6H11OH) needed to produce 45.0 g cyclohexene (C6H10) if the reaction has a 86.2%
(A) Nitric acid, HNO3 is produced from ammonia and oxygen by the consecutive reactionsHow many grams of nitric acid can be obtained from 1.00 kg NH3(g), if NO(g) in the third reaction is not recycled?(B) Nitrogen gas is used to inflate automobile air bags. The gas is produced by detonation of a
A 3.104 g sample of an oxide of manganese contains 1.142 grams of oxygen. Write a balanced chemical equation for the reaction that produces the compound from Mn(s) and O2(g).
Titanium dioxide, TiO2 is the most widely used white pigment for paints, having displaced most lead-based pigments, which are environmental hazards. Before it can be used, however, naturally occurring TiO2 must be freed of colored impurities. One process for doing this converts impure TiO2(s) , to
Iron metal reacts with chlorine gas. How many grams of FeCl3 are obtained when 515 g Cl2 reacts with excess Fe?2 Fe(s) + 3 Cl2(g) → 2 FeCl3(s)
If 75.8 g PCl3 is produced by the reaction6 Cl2(g) + P4(s) → 4 PCl3(l)how many grams each of Cl2 and P4 are consumed?
A 0.696 mol sample of Cu is added to 136 mL of 6.0 M HNO3. Assuming the following reaction is the only one that occurs, will the Cu react completely?3 Cu(s) + 8 HNO3(aq) → 3 Cu(NO3)2(aq) + 4 H2O(l) + 2 NO(g)
Titanium tetrachloride, TiCl4, is prepared by the reaction below.3 TiO2(s) + 4 C(s) + 6 Cl2(g) → 3 TiCl4(g) + 2 CO2(g) + 2 CO(g)What is the maximum mass of TiCl4 that can be obtained from 35 g TiO2, 45 g Cl2, and 11 g C?
In the reaction of 277 g CCl4 with an excess of HF, 187 g CCl2F2 is obtained. What are the (a) Theoretical,(b) Actual, and (c) Percent yields of this reaction?CCl4 + 2 HF→CCl2F2 + 2 HCl
How many grams of commercial acetic acid (97% CH3COOH by mass) must be allowed to react with an excess of PCl3 to produce 75 g of acetyl chloride (CH3COCl), if the reaction has a 78.2% yield?CH3COOH + PCl3 → CH3COCl + H3PO3 (not balanced)
Suppose that reactions (a) and (b) each have a 92% yield. Starting with 112 g CH4 in reaction (a) and an excess of Cl2(g), how many grams of CH2Cl2 are formed in reaction (b)?(a) CH4 + Cl2→CH3Cl + HCl(b) CH3Cl + Cl2→CH2Cl2 + HCl
An essentially 100% yield is necessary for a chemical reaction used to analyze a compound, but it is almost never expected for a reaction that is used to synthesize a compound. Explain this difference.
Suppose we carry out the precipitation of Ag2CrO4(s) described in Example 4-10. If we obtain 2.058 g of precipitate, we might conclude that it is nearly pure Ag2CrO4 but if we obtain 2.112 g, we can be quite sure that the precipitate is not pure. Explain this difference.Example 4-10A 25.00 mL
How many grams of HCl are consumed in the reaction of 425 g of a mixture containing 35.2% MgCO3 and 64.8% Mg(OH)2, by mass? Mg(OH)2 + 2 HCl → MgCl2 + 2 H2OMgCO3 + 2 HCl → MgCl2 + H2O + CO2
How many grams of CO2 are produced in the complete combustion of 406 g of a bottled gas that consists of 72.7% propane(C3H8) and 27.3% butane (C4H10), by mass?
Dichlorodifluoromethane, once widely used as a refrigerant, can be prepared by the reactions shown. How many moles of Cl2 must be consumed in the first reaction to produce 2.25 kg CCl2F2 in the second? Assume that all the CCl4 produced in the first reaction is consumed in the second. CH4 + Cl2 →
Carbon dioxide gas, CO2(g), produced in the combustion of a sample of ethane is absorbed in Ba(OH)2(aq), producing 0.506 g BaCO3(s). How many grams of ethane (C2H6) must have been burned? C2H6(g) + O2(g) → CO2(g) + H2O(l) (not balanced) CO2(g) + Ba(OH)2(aq) → BaCO3(s) + H2O(l)
The following process has been used to obtain iodine from oil-field brines in California. How many kilograms of silver nitrate are required in the first step for every kilogram of iodine produced in the third step? sodium iodide + silver nitrate → silver iodide + sodium nitrate silver iodide +
A fundamental principle in green chemistry is atom economy (AE). AE is a measure of how many atoms from the starting materials are incorporated into the desired product. For example, if a reaction incorporates all the reactant atoms into the product of interest, the reaction has a percent AE of
The formula for calcium chlorite is (a) CaClO2;(b) Ca(ClO2)2; (c) CaClO3;(d) Ca(ClO4)2.
A formula unit of the compound [Cu(NH3)4]SO4 has nearly equal masses of (a) S and O; (b) N and O;(c) H and N; (d) Cu and O.
An isomer of the compound CH3CH2CHOHCH3 is(a) C4H10O; (b) CH3CHOHCH2CH3;(c) CH3(CH2)2OH; (d) CH3CH2OCH2CH3.
A hydrate of Na2SO3 contains almost exactly 50% H2O by mass. What is the formula of this hydrate?
Malachite is a common copper-containing mineral with the formula CuCO3 · Cu(OH)2. (a) What is the mass percent copper in malachite? (b) When malachite is strongly heated, carbon dioxide and water are driven off, yielding copper(II) oxide as the sole product. What mass of copper(II) oxide is
Acetaminophen, an analgesic and antipyretic drug, has a molecular mass of 151.2 u and a mass percent composition of 63.56% C, 6.00% H, 9.27% N, and 21.17% O. What is the molecular formula of acetaminophen?
Ibuprofen is a compound used in painkillers. When a 2.174 g sample is burned in an excess of oxygen, it yields 6.029 g CO2 and 1.709 g H2O as the sole products. (a) What is the percent composition, by mass, of ibuprofen? (b) What is the empirical formula of ibuprofen?
Balance the following equations by inspection.(a) SO3 → SO2 + O2(b) Cl2O7 + H2O → HClO4(c) NO2 + H2O → HNO3 + NO(d) PCl3 + H2O → H3PO3 + HCl.
Liquid triethylene glycol is used as a solvent and plasticizer for vinyl and polyurethane plastics. Write a balanced chemical equation for the combustion of this compound in a plentiful supply of oxygen. A ball-and-stick model of triethylene glycol is shown here. Triethylene glycol
(A) Write a balanced equation to represent the reaction of mercury(II) sulfide and calcium oxide to produce calcium sulfide, calcium sulfate, and mercury metal.(B) Write a balanced equation for the combustion of thiosalicylic acid, C7H6O2S, used in the manufacture of indigo dyes. A ball-and- stick
Sodium nitrite is used in the production of dyes for coloring fabrics, as a preservative in meat processing (to prevent botulism), as a bleach for fibers, and in photography. It can be prepared by passing nitrogen monoxide and oxygen gases into an aqueous solution of sodium carbonate. Carbon
For the elements K, Cl, and O in the following equations, the requirement that the number of atoms be equal on either side of the equation is met. Why is none of them an acceptable balanced equation for the decomposition of solid potassium chlorate yielding solid potassium chloride and oxygen
Balance the following equations by inspection.(a) P2H4 → PH3 + P4(b) P4 + Cl2 → PCl3(c) FeCl3 + H2S → Fe2S3 + HCl(d) Mg3N2 + H2O → Mg(OH)2 + NH3.
(A) For an initial reaction mixture containing 0.500 mol Fe(s) and 0.500 mol H2O(g), what is the maximum possible value for the extent of reaction, ? The chemical equation for the reaction is 3 Fe(s) + 4 H2O(g) → Fe3O4(s) + 4 H2(g).(B) Consider the reaction 2 N2 + 3 O2 + 4 HCl → 4 NOCl + 2 H2O.
A commercial method of manufacturing hydrogen involves the reaction of iron and steam.(a) How many grams of H2 can be produced from 87.2 g Fe and an excess of H2O(g) (steam)?(b) How many grams of H2O are consumed in the conversion of 25.0 g Fe to Fe3O4?(c) If 29.2 g H2 is produced, how many grams
(a) Determine the stoichiometric numbers for the following reaction, which occurs to a limited extent at 25 °C: 4 KO2(s) + 2 CO2(g) → 2 K2CO3(s) + 3 O2(g).(b) In an experiment carried out at 25 °C, a reaction mixture containing 2.478 mol KO2 and 0.979 mol CO2 yields 1.128 mol O2. Calculate the
How many grams of Ag2CO3 are decomposed to yield 75.1 g Ag in this reaction? Ag2CO3(s) Ag(s) + CO₂(g) + O₂(g) (not balanced)
(A) Hexamethylenediamine has the molecular formula C6H16N2. It is one of the starting materials for the production of nylon. It can be prepared by the following reaction:C6H10O4(l) + NH3(g) + H2(g) → C6H16N2(l) + H2O(l) (not balanced)A large reaction vessel contains 4.15 kg C6H10O4, 0.547 kg NH3,
How many kilograms of HNO3 are consumed to produce 125 kg Ca(H2PO4)2 in this reaction? Ca3(PO4)2 + HNO3 → Ca(H2PO4)2 + Ca(NO3)2 (not balanced)
The reaction of calcium hydride with water can be used to prepare small quantities of hydrogen gas, as is done to fill weather-observation balloons.CaH2(s) + H2O(l) → Ca(OH)2(s) + H2(g) (not balanced)(a) How many grams of H2(g) result from the reaction of 127 g CaH2 with an excess of water?(b)
The reaction of potassium superoxide, KO2, is used in life-support systems to replace CO2(g) in expired air with O2(g). The unbalanced chemical equation for the reaction is given below.KO2(s) + CO2(g) → K2CO3(s) + O2(g)(a) How many moles of O2(g) are produced by the reaction of 88.0 g CO2(g) with
Iron ore is impure Fe2O3. When Fe2O3 is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are produced. From a sample of ore weighing 938 kg, 523 kg of pure iron is obtained. What is the mass percent Fe2O3 in the ore sample, assuming that none of the impurities contain
Solid silver oxide, Ag2O(s), decomposes at temperatures in excess of 300 °C, yielding metallic silver and oxygen gas. A 3.13 g sample of impure silver oxide yields 0.187 g O2(g). What is the mass percent Ag2O in the sample? Assume that Ag2O(s) is the only source of O2(g).
Decaborane, B10H14, was used as a fuel for rockets in the 1950s. It reacts violently with oxygen, O2, to produce B2O3 and water. Calculate the percentage by mass of B10H14 in a fuel mixture designed to ensure that B10H14 and O2 run out at exactly the same time.
A piece of aluminum foil measuring 10.25 cm X 5.50 cm X 0.601 mm is dissolved in excess HCl(aq). What mass of H2(g) is produced? Use equation (4.2) and d = 2.70 g/cm3 for Al.Eq. 4.2 2 Al(s) + 6 HCl(aq) 2 AlCl3(aq) + 3 H₂(g) (4.2)
The rocket boosters of the space shuttle Discovery, launched on July 26, 2005, used a fuel mixture containing primarily solid ammonium perchlorate, NH4ClO4(s), and aluminum metal. The unbalanced chemical equation for the reaction is given below.Al(s) NH4ClO4(s) → Al2O3(s) + AlCl3(s) +H2O(l)+
An excess of aluminum foil is allowed to react with 225 mL of an aqueous solution of HCl (d = 1.088 g/mL) that contains 18.0% HCl by mass. What mass of H2(g) is produced?
Without performing detailed calculations, which of the following metals yields the greatest amount of H2 per gram of metal reacting with HCl(aq)? (a) Na, (b) Mg,(c) Al, (d) Zn.
Without performing detailed calculations, which of the following yields the same mass of CO2(g) per gram of compound as does ethanol, CH3CH2OH, when burned in excess oxygen? (a) H2CO;(b) HOCH2CH2OH;(c) HOCH2CH;(d) CH3OCH3; (e) C6H5OH.
What are the molarities of the following solutes when dissolved in water?(a) 2.92 mol CH3OH in 7.16 L of solution(b) 7.69 mmol CH3CH2OH in 50.00 mL of solution(c) 25.2 g CO(NH2)2 in 275 mL of solution.
What are the molarities of the following solutes when dissolved in water?(a) 2.25 x 10-4 mol CH3CH2OH in 125 mL of solution(b) 57.5 g (CH3)2CO in 525 mL of solution(c) 18.5 mL of C3H5(OH)3 (d = 1.26 g/mL) in 375 mL of solution.
What are the molarities of the following solutes?(a) Sucrose C12H22O11) if 150.0 g is dissolved per 250.0 mL of water solution(b) Urea, CO(NH2)2, if 98.3 mg of the 97.9% pure solid is dissolved in 5.00 mL of aqueous solution(c) Methanol, CH3OH, (d = 0.792 g/mL) if 125.0 mL is dissolved in enough
What are the molarities of the following solutes?(a) Aspartic acid (H2C4H5NO4) if 0.405 g is dissolved in enough water to make 100.0 mL of solution(b) Acetone, (CH3)2CO, (d = 0.790 g>mL) if 35.0 mL is dissolved in enough water to make 425 mL of solution(c) Diethyl ether, (C2H5)2O, if 8.8 mg is
How much(a) Glucose, C6H12O6 in grams, must be dissolved in water to produce 75.0 mL of 0.350 M C6H12O6?(b) Methanol, CH3OH (d = 0.792 g/mL), in milliliters, must be dissolved in water to produce 2.25 L of 0.485 M CH3OH?
How much(a) Ethanol, CH3CH2OH (d = 0.789 g/mL), in liters, must be dissolved in water to produce 200.0 L of 1.65 M CH3CH2OH?(b) Concentrated hydrochloric acid solution (36.0% HCl by mass; d = 1.18 g/mL), in milliliters, is required to produce 12.0 L of 0.234 M HCl?
In many communities, water is fluoridated to prevent tooth decay. In the United States, for example, more than half of the population served by public water systems has access to water that is fluoridated at approximately 1 mg F per liter. (a) What is the molarity of F in water if it contains 1.2
Which of the following is a 0.500 M KCl solution?(a) 0.500 g KCl/mL solution; (b) 36.0 g KCl/L solution;(c) 7.46 mg KCl/mL solution; (d) 373 g KCl in 10.00 L solution.
Which two solutions have the same concentration?(a) 55.45 g NaCl/L solution; (b) 5.545 g NaCl/100 g solution; (c) 55.45 g NaCl/kg water;(d) 55.45 mg NaCl/1.00 mL solution; (e) 5.00 mmol NaCl/5.00 mL solution.
Which has the higher concentration of sucrose: a 46% sucrose solution by mass (d = 1.21 g/mL), or 1.50 M C12H22O11? Explain your reasoning.
Which has the greater molarity of ethanol: a white wine (d = 0.95 g/mL) with 11% CH3CH2OH by mass, or the solution described in Example 4-7? Explain your reasoning.Example 4-7A solution is prepared by dissolving 25.0 mL ethanol, CH3CH2OH (d = 0.789 g/mL), in enough water to produce 250.0 mL
A 10.00 mL sample of 2.05 M KNO3 is diluted to a volume of 250.0 mL. What is the concentration of the diluted solution?
What volume of 2.00 M AgNO3 must be diluted with water to prepare 500.0 mL of 0.350 M AgNO3?
Water is evaporated from 125 mL of 0.198 M K2SO4 solution until the volume becomes 105 mL. What is the molarity of K2SO4 in the remaining solution?
A 25.0 mL sample of HCl(aq) is diluted to a volume of 500.0 mL. If the concentration of the diluted solution is found to be 0.085 M HCl, what was the concentration of the original solution?
Given a 0.250 M K2CrO4 stock solution, describe how you would prepare a solution that is 0.0125 M K2CrO4. That is, what combination(s) of pipet and volumetric flask would you use? Typical sizes of volumetric flasks found in a general chemistry laboratory are 100.0, 250.0, 500.0, and 1000.0 mL, and
Given two liters of 0.496 M KCl, describe how you would use this solution to prepare 250.0 mL of 0.175 M KCl. Give sufficient details so that another student could follow your instructions.
Consider the reaction below:2 AgNO3(aq) + Na2S(s) → Ag2S(s) + 2 NaNO3(aq)(a) How many grams of Na2S(s) are required to react completely with 27.8 mL of 0.163 M AgNO3?(b) How many grams of Ag2S(s) are obtained from the reaction in part (a)?
Excess NaHCO3 is added to 525 mL of 0.220 M Cu(NO3)2. These substances react as follows:Cu(NO3)2(aq) + 2 NaHCO3(s) → CuCO3(s) + 2 NaNO3(aq) + H2O(l) + CO2(g)(a) How many grams of the NaHCO3(s) will be consumed?(b) How many grams of CuCO3(s) will be produced?
How many milliliters of 0.650 M K2CrO4 are needed to precipitate all the silver in 415 mL of 0.186 M AgNO3 as Ag2CrO4(s)?2 AgNO3(aq) + K2CrO4(aq) → Ag2CrO4(s) + 2 KNO3(aq)
Consider the reaction below.Ca(OH)2(s) + 2 HCl(aq) → CaCl2(aq) + 2 H2O(l)(a) How many grams of Ca(OH)2 are required to react completely with 415 mL of 0.477 M HCl?(b) How many kilograms of Ca(OH)2 are required to react with 324 L of a HCl solution that is 24.28% HCl by mass, and has a density of
Exactly 1.00 mL of an aqueous solution of HNO3 is diluted to 100.0 mL. It takes 29.78 mL of 0.0142 M Ca(OH)2 to convert all of the HNO3 to Ca(NO3)2. The other product of the reaction is water. Calculate the molarity of the undiluted HNO3 solution.
Refer to Example 4-6 and equation (4.2). For the conditions stated in Example 4-6, determine (a) The number of moles of and (b) The molarity of the if the solution volume is simply the 23.8 mL calculated in the example.Example 4-6A hydrochloric acid solution consists of 28.0% HCl by mass and has
A 5.00 mL sample of an aqueous solution of H3PO4 requires 49.1 mL of 0.217 M NaOH to convert all of the H3PO4 to Na2HPO4. The other product of the reaction is water. Calculate the molarity of the H3PO4 solution.
Refer to the Integrative Example on page 140. If 138 g Na2CO3 in 1.42 L of aqueous solution is treated with an excess of NO(g) and O2(g), what is the molarity of the NaNO2(aq) solution that results? Integrative Ex.Sodium nitrite is used in the production of dyes for coloring fabrics, as a
How many grams of Ag2CrO4 will precipitate if excess K2CrO4(aq) is added to the 415 mL of 0.186 M AgNO3 in Exercise 51?Exercise 51How many milliliters of 0.650 M K2CrO4 are needed to precipitate all the silver in 415 mL of 0.186 M AgNO3 as Ag2CrO4(s)?2 AgNO3(aq) + K2CrO4(aq) → Ag2CrO4(s) + 2
What volume of 0.0665 M KMnO4 is necessary to convert 12.5 g KI to I2 in the reaction below? Assume that H2SO4 is present in excess.2 KMnO4 + 10 KI + 8 H2SO4 → 6 K2SO4 + 2 MnSO4 + 5 I2 + 8 H2O
How many grams of sodium must react with 155 mL H2O to produce a solution that is 0.175 M NaOH?2 Na(s) + 2 H2O(l)¡2 NaOH(aq) + H2(g)
A method of lowering the concentration of HCl(aq) is to allow the solution to react with a small quantity of Mg. How many milligrams of Mg must be added to 250.0 mL of 1.023 M HCl to reduce the solution concentration to exactly 1.000 M HCl?Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
How many moles of NO(g) can be produced in the reaction of 3.00 mol NH3(g) and 4.00 mol O2(g)? 4 NH3(g) + 5O₂(g) 4 NO(g) + 6 H₂0(1)
A 0.3126 g sample of oxalic acid, H2C2O4 requires 26.21 mL of a particular concentration of NaOH(aq) to complete the following reaction. What is the molarity of the NaOH(aq)?H2C2O4(s) + 2 NaOH(aq)→Na2C2O4(aq) + 2 H2O(l)
The reaction of calcium hydride and water produces calcium hydroxide and hydrogen as products. How many moles of H2(g) will be formed in the reaction between 0.82 mol CaH2(s) and 1.54 mol H2O(l)?
How many grams of H2(g) are produced by the reaction of 1.84 g Al with 75.0 mL of 2.95 M HCl?
Lithopone is a brilliant white pigment used in water based interior paints. It is a mixture of BaSO4 and ZnS produced by the reactionHow many grams of lithopone are produced in the reaction of 315 mL of 0.275 M ZnSO4 and 285 mL of 0.315 M BaS? BaS(aq) + ZnSO4(aq) → ZnS(s) + BaSO4(s) lithopone
A side reaction in the manufacture of rayon from wood pulp is 3 CS2 + 6 NaOH → 2 Na2CS3 + Na2CO3 + 3 H2O How many grams of Na2CS3 are produced in the reaction of 92.5 mL of liquid CS2 (d = 1.26 g/mL) and 2.78 mol NaOH?
Ammonia can be generated by heating together the solids NH4Cl and Ca(OH)2. CaCl2 and H2O are also formed. (a) If a mixture containing 33.0 g each of NH4Cl and Ca(OH)2 is heated, how many grams of NH3 will form? (b) Which reactant remains in excess, and in what mass?

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