2Fe(OH)3(s) + 3H2SO4(aq) Fe2(SO4)3(aq) + 6H2O(l) If 2.4 g Fe(OH)3 and 3.3 g H2SO4 react and make 4.5 g Fe2(SO4)3, ____ g H2O are made also. Find theoretical yield of Fe2(SO4)3 in a reaction of 24.1 mol Fe(OH)3 and 30.5 mol H2SO4 : The theoretical yield of Fe2(SO4)3 is ____________ moles If only 8.2 mol Fe2(SO4)3 was isolated, the percent reaction yield is ________%

2Fe(OH)3(s) + 3H2SO4(aq) Fe2(SO4)3(aq) + 6H2O(l) If 2.4 g Fe(OH)3 and 3.3 g H2SO4 react and make 4.5 g Fe2(SO4)3, g H2O are made also. Find theoretical yield of Fe2(SO4)3 in a reaction of 24.1 mol Fe(OH)3 and 30.5 mol H2SO4 : The theoretical yield of Fe2(SO4)3 is moles If only 8.2 mol Fe2(SO4)3 was isolated, the percent reaction yield is %

General Chemistry - Standalone book (MindTap Course List)

11th Edition

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

Chapter3: Calculations With Chemical Formulas And Equaitons

Section: Chapter Questions

Problem 3.26QP

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2Fe(OH)3(s) + 3H2SO4(aq) Fe2(SO4)3(aq) + 6H2O(l) If 2.4 g Fe(OH)3 and 3.3 g H2SO4 react and make 4.5 g Fe2(SO4)3, ____ g H2O are made also. Find theoretical yield of Fe2(SO4)3 in a reaction of 24.1 mol Fe(OH)3 and 30.5 mol H2SO4 : The 24.1 mol Fe(OH)3 are enough to form ____________ mol Fe2(SO4)3.The 30.5 mol H2SO4 are enough to form ____________ mol Fe2(SO4)3.The limiting reagent in the mixture is _____
Titanium dioxide (TIO2) is a white molecule that is used as a pigment for white paint. It is produced industrially by treating a mineral called ilmenite (FeTiO3) with sulfuric acid according the molecular equation below. In one particular reaction, 8,000 Kg of FeTiO3was used as a starting material for the reaction. What is the theoretical yield of TiO2? MW FeTiO3= 151.72 g/mol, MW TiO2= 79.88 g/mol. FeTiO3+ H2SO4→ TiO2+ FeSO4+ H2O
91. Ammonia reacts with O₂ to form either NO(g) or NO₂(g) according to the following UNBALANCED equations: NH₃(g) + O₂(g) → NO(g) + H₂O(g) NH₃(g) + O₂(g) → NO₂(g) + H₂O(g) In one experiment 6.00 moles of NH₃(g) and 15.00 moles of O₂(g) were placed in a closed flask and allowed to react. After the reaction was complete, 6.75 moles of O₂(g) remained and all of the NH₃(g) had reacted. Calculate the number of moles of NO(g) formed in the reaction mixture.
2). H2S and SO2 as follows,(8pt) H2S + SO2 ------>S + H2O In a particular experiment, 7.95 g of sulfur is produced by the reaction of 7.5 g of H2S with 12.75 g of SO2. What is the % yield of sulfur?
Consider the reaction. 2Al(s)+Fe2O3(s)−→−heatAl2O3(s)+2Fe(l)2Al(s)+Fe2⁢O3⁡(s)→heatAl2⁢O3⁡(s)+2Fe(l) If 18.3 kg Al18.3 kg Al reacts with an excess of Fe2O3,Fe2⁢O3, how many kilograms of Al2O3Al2⁢O3 will be produced? mass of Al2O3Al2⁢O3 produced:
Phosporic acid (H3PO4) is a key ingredient in soft drinks that gives it a sharper flavor. One way to produce thic acid is with the aid of mineral fluoroapatite (Ca5(PO4)3F following this reaction Ca5(PO4)3F + 5H2SO4 -> 3H3PO4 + 5CaSO4 + HF If 24.5 g Ca5(PO4)3F is mixed with 89.7 g H2SO4, how much H3PO4 will form?
Silicon tetrachloride (SIC14) can be prepared by heating Si in chlorine gas: Si(s) + 2Cl₂(g)-> SiCl4(1) in one reaction, 0.507 mole of SiC14 is produced. What mass (grams) of molecular chlorine were used in the reaction? Choose the nearest answer. MW SIC14-169.9 g/mol: MW Cl = 35.453g /mol
Consider the balanced chemical reaction: 2Al+3Br2-----2AlBr3 If 6.0 g of aluminum reacts with 68 g of bromine and the reaction has an 85% yield, how many grams of aluminum bromide can you form? a. Theoretical yield of AlBr3= ? b. Actual yield of AlBr3=?
Aluminium reacts with iodine according to the following equation: 2Al(s) + 3I2(s) → Al2 I6(s) a. How many moles of Al2 I6 are produced by the reaction of 4.0 mole of aluminium? b. How many moles of I2 are required to react exactly with 0.429 mole of aluminium?
When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. Condition #1: C(s) + O2 (g) --> CO2 (g) However, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. Condition #2: 2 C(s) + O2 (g) -->2 CO (g) What mass of CO (g) and CO2 (g) is expected when a 5.00 gram sample of pure carbon is burned under each of these two conditions listed above? Condition #1: Condition #2:
When 5.82 g of magnesium nitride is place in 9.73 g water, the reaction is: Mg3N2 + H2O → NH3 + MgO (Unbalanced Equation) (Atomic Weights: Mg=24.3, N=14, H=1, O=16) 1.Which reactant is limiting? 2.How many grams of ammonia are produced? 3. How many grams of magnesium oxide are produced?
Ammonia reacts with O2 to form either NO(g) or NO2 (g) according to the following UNBALANCED equations: NH3 (g) + O2 (g) → NO(g) + H2O(g) NH3(g) + O2(g) → NO2 (g) + H2O(g) In one experiment 6.00 moles of NH(g) and 15.00 moles of O2 (g) were placed in a closed flask and allowed to react. After the reaction was complete, 5.55 moles of O2 (g) remained and all of the NH3 (g) had reacted. Calculate the number of moles of NO(g) formed in the reaction mixture.

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General Chemistry - Standalone book (MindTap Cour…

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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