Aluminum hydroxide reacts with sulfuric acid as follows:2 Al(OH)3(s) + 3 H2SO4(aq)Al2(SO4)3 (aq) + 6 H20(1)a. Which is the limiting reactant when 0.500 mol Al(OH)3 and 0.500 mol H2SO4 are allowedto react?b. How many moles of Al2(SO4)3 can form under these conditions?c. How many moles of the excess reactant remain after the completion of the reaction?

Aluminum hydroxide reacts with sulfuric acid as follows: 2 Al(OH)3(s) + 3 H2SO4(aq) Al2(SO.)3 (aq) + 6 H2O(1) a. Which is the limiting reactant when 0.500 mol Al(OH)3 and 0.500 mol H2SO, are allowed to react? b. How many moles of Al2(SO.)3 can form under these conditions? c. How many moles of the excess reactant remain after the completion of the reaction?

Aluminum hydroxide reacts with sulfuric acid as follows: 2 Al(OH)3(s) + 3 H2SO4(aq) Al2(SO.)3 (aq) + 6 H2O(1) a. Which is the limiting reactant when 0.500 mol Al(OH)3 and 0.500 mol H2SO, are allowed to react? b. How many moles of Al2(SO.)3 can form under these conditions? c. How many moles of the excess reactant remain after the completion of the reaction?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 53QAP: Cyanogen gas, C2N2, has been found in the gases of outer space. It can react with fluorine to form...

See similar textbooks

Similar questions

A friend asks if you would be willing to check several homework problems to see if she is on the right track. Following are the problems and her proposed solutions. When you identify the problem with her work, make the appropriate correction. a Calculate the number of moles of calcium in 27.0 g of Ca. 27.0gCa1molCa6.0221023gCa=? b Calculate the number of potassium ions in 2.5 mol of K2SO4. 2.5molK2SO41molK+ions1molK2SO46.0221023K+ions1molK+ions=? c Sodium reacts with water according to the following chemical equation. 2Na+2H2OH2+2NaOH Assuming complete reaction, calculate the number of moles of water required to react with 0.50 mol of Na. 0.50molNa1molH2O2molNa=?
4.33 Silicon carbide, an abrasive, is made by the reaction of silicon dioxide with graphite (solid carbon): SiO2+CSiC+CO(balanced?) We mix 150.0 g of SiO2 and 101.5 g of C. If the reaction proceeds as far as possible, which reactant is left over? How much of this reactant remains?
Ethylene oxide, C2H4O, is made by the oxidation of ethylene, C2H4. 2C2H4(g)+O2(g)2C2H4O(g) Ethylene oxide is used to make ethylene glycol for automobile antifreeze. In a pilot study, 10.6 g of ethylene gave 9.91 g of ethylene oxide. What is the percentage yield of ethylene oxide?
Urea [(NH2)2CO] is a by-product of protein metabolism, and it can be synthesized in a lab by combining ammonia and carbon dioxide according to the following equation: 2NH3(g) + CO2(g) ⟶⟶ (NH2)2CO(aq) + H2O(l) a) Determine the moles of carbon dioxide required to reaction with 2.50 moles of ammonia. ? moles CO2 b) How many moles of urea will be produced by the complete reaction of 2.50 moles of ammonia? ? moles urea
Nitric acid (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark brown gas: 2NO(g) + O2(g) → 2NO2(g) In one experiment 0.886 mole of NO is mixed with 0.503 mol of O2. a. Calculate which of the two reactants is the limiting reagent.b. Calculate also the number of moles of NO2 produced. c. What reactant is left over and how much of it is left over?
Ferric chloride, FeCl3 reacts with silver nitrate, AgNO3 to form ferric nitrate, Fe (NO3)3 and silver chloride, AgCl. a. Write the balanced chemical equation of the reaction. b. If 108.5 moles of FeCl3 is combined with 76.8 moles of AgNO3, how many moles of AgCl is produced? c. How many grams of AgCl is produced? d. Which reactant is the limiting reagent? e. Which reactant is the excess reagent?
3. Nitrogen monoxide (NO) is an intermediate product in the production of nitric acid from ammonia (NH3) and oxygen gas. 4 NH3 + 5 O2 ——> 4 NO + 6H20 a. Which is the limiting and excess reactant? b. What maximum amount of nitrogen monoxide can be produced from 68.0 g NH3 and 216 g O2? c. How many moles of the excess reactant was used? d. How much of the excess reactant was left? e. If the reaction produced 98.0 g nitrogen monoxide, what is the percent yield of the reaction?
1.) 1.87 g of acetic acid (vinegar, C2H4O2) reacts with 2.13 g of isopentyl alcohol (C5H12O) to yield isopentyl acetate (C7H14O2), a fragrant substance with the odor of bananas. The reaction is: C2H4O2 + C5H12O ⎯→ C7H14O2 + H2O a.) Which are the limiting reactant (LR) and excess reactant (ER)? b.) How many grams of isopentyl acetate was formed? c.) How many grams of the excess reactant are left after the reaction is complete? d.) If 2.96 g of isopentyl acetate was produced, what is the % yield of the reaction?
4. The depletion of ozone (O3) in the stratosphere has been a matter of great concern among scientists in recent years. It is believed that ozone can react with nitric oxide (NO) that is discharged from high altitude planes. The reaction is O3 + NO à O2 + NO2 If 7.40 g of O3 reacts with 0.670 g of NO, a) Which compound will be the limiting reagent? b) How many grams of NO2 will be produced? g (3 decimal places) c) Calculate the number of moles of the excess reagent remaining at the end of the reaction. mol (4 decimal places)
Certain salts of benzoic acid have been used as food additives for decades. The potassium salt of benzoic acid, potassium benzoate, can be made by the action of potassium permanganate on toluene according to the following reaction (unbalanced): C7H8 + KMnO4  KC7H5O2 + MnO2 + KOH + H2O What is the limiting reactant when 10.409 g of toluene react with 14.366 g of potassium permanganate?
Sulfuric acid is formed in the atmosphere by the reaction of sulfur dioxide and oxygen gas on the surface of water droplets: SO2(g) + H2O(l) + O2(g) ⟶ H2SO4(aq) When 2.6 moles of SO2 reacts with 3.0 moles of H2O and 2.9 moles of O2, [ Select ] ["H2O", "SO2", "O2"] is the limiting reactant, and [ Select ] ["O2 and SO2", "SO2 and H2O", "O2 and H2O"] are present in excess
For the reaction N2 + 3H2 = 2NH3, if you have 2.00 moles N2 and 4.00 of H2: How many moles of NH3 can be formed, and how many moles of excess reactant will remain?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS