2. ) 50.94g/mol4V(s) +32.00 g/mol302(g)149.88g/mol2V203(s)a. Calculate the theoretical yield of vanadium (III) oxide, assuming you begin with 220grams of vanadium metal.b. When this experiment is performed by researcher, an experimental yield 182.0grams is produced. Calculate the percent yield.

Given reaction is : 4V (s) + 3O2 (g) --------> 2V2O3 (s) Gram molar mass of V = 50.94 g/mole…

Answered: 32.00 g/mol 149.88g/mol 2. ) 50.94g/mol…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 68P

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Outline the steps needed to solve the following problem, then do the calculations. Ether, (C2H5)2O, which was originally used as an anesthetic but has been replaced by safer and more effective medications, is prepared by the reaction of ethanol with sulfuric acid. 2C2H5OH+H2SO4(C2H5)2O+H2SO4H2O What is the percent yield of ether if 1.17 L (d = 0.7134 g/mL) is isolated from the reaction of 1.500 L of C2H5OH (d = 0.7894 g/mL)?
Phosphoric acid, one of the acids used in some cola drinks, is produced by the reaction of phosphorus(V) oxide, an acidic oxide, with water. Phosphorus(V) oxide is prepared by the combustion of phosphorus. (a) Write the empirical formula of phosphorus(V) oxide. (b) What is the molecular formula of phosphorus(V) oxide if the molar mass is about 280. (c) Write balanced equations for the production of phosphorus(V) oxide and phosphoric acid. (d) Determine the mass of phosphorus required to make 1.00104 kg of phosphoric acid, assuming a yield of 98.35%.
How many grams of solid Ca3(PO4)2 can be formed from a reaction of 51.8 mL of 0.754 M CaCl2 and 21.5 mL of 1.04 M Na3PO4? Why can't 4.04 g of solid Ca3(PO4)2 be formed under these conditions? This amount is (greater than, less than, or equal to) the theoretical yield.
Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures: 5Ca + V2O5 5CaO + 2V In one process, 1.540 ×103 g of V2O5 react with 1.960 × 103 g Ca. (a) Calculate the theoretical yield of V. (b) Calculate the percent yield if 769.0 g of V are obtained.
1.736 g of iron ore is dissolved with acid and precipitated as Fe2O3X.H2O. After the precipitate is filtered and washed, it is converted to Fe2O3. If the weight of Fe2O3 is 0.248 g, calculate the percentage of Fe in the sample?
Bi2O3 is a basic oxide. Write a balanced chemical equation for its reaction with dilute nitric acid. If 6.77 g ofBi2O3 is dissolved in dilute acidic solution to make 0.500 L of solution, what is the molarity of the solution ofBi3 + ion?
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A 0.896 g sample of impure magnesite, MgCO3 , was decomposed with HCl; the liberated CO2 was collected on calcium oxide and found to weigh 0.2881 g. Calculate the percentage of magnesium in the sample.
An iron ore was analyzed by dissolving a 1.957-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron(III) was precipitated as the hydrous oxide Fe2O3·xH2O by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.6009 g of pure Fe2O3. Calculate (a) the % Fe and (b) the % Fe3O4 in the sample.
Potassium superoxide, KO2, is often used in oxygen masks(such as those used by firefighters) because KO2 reacts withCO2 to release molecular oxygen. Experiments indicate that 2mol of KO2(s) react with each mole of CO2(g). (a) The productsof the reaction are K2CO3(s) and O2(g). Write a balanced equationfor the reaction between KO2(s) and CO2(g). (b) Indicatethe oxidation number for each atom involved in the reactionin part (a). What elements are being oxidized and reduced?(c) What mass of KO2(s2) is needed to consume 18.0 g CO2(g)?What mass of O2(g) is produced during this reaction?
A 0.896 g sample of impure magnesite, MgCO3, was decomposed with HCl; the liberated CO 2 was collected on calcium oxide and found to weigh 0.2881 g. Calculate the percentage of magnesium in the sample.

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