Vanadium metal reacts with oxygen to produce vanadium(V) oxide, V2O5. What amount of V2 05 can be produced from the reaction of0.340 mol V, and what amount of O2 is consumed? Fill in the amounts table with your responses.4 V(s)5 O2(g)2 V2O5 (s)->EquationInitial (mol)0.340-0.340Change (mol)Final (mol)Submit AnserTry Anoder ersion10:28 AM3/4/2020FLVhere to search

Given: Initial moles of Vanadium (V) = 0.340 mol Balanced chemical reaction is given by,

Answered: Vanadium metal reacts with oxygen to…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 161IP: In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric...

See similar textbooks

Similar questions

According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
8. Write the net ionic equation for cach reaction. a. K;CO;(aq) + CaCl:(aq) → CaCO;(s) + 2KCI(aq) b. Pb(NO3):(aq) + (NH,);S(aq) → 2NH,NO;(aq) + PbS(s) 2LİCI(aq) + 2Hg.(NO,)(aq) → Hg,Cl;(s) + 2LİNO;(aq) d. 2NAOH(aq) + MgCl;(aq) -AMg(OH):(s) + 2NaCl(aq) 2011 Cengage Leaning All Rights Reserves May tiet beseanned.copied.or duplicated, or posted to a publicly accessible websi Chapter 7: Reactions in A 33,765)
When exactly 750.0 mL of a solution containing 580.4 ppm of calcium nitrate was combined with 200.0 mL of a solution containing 0.08090 M of boron sulfate (a), how much solid CaSO4 was formed in grams? (b) What was the unreacted reagents' molar concentration? (MM of Ca=40.078; N-14; O-16; B-10.81; S-32.065)
Be sure to answer all parts. Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with caleium at high temperatures: 5Ca + V,0g → 5C2O + 2V In one process, 1.540 × 10° g of V,Og react with 2.040 × 10° g Ca. (a) Calculate the theoretical yield of V. (b) Calculate the percent yield if 781.0 g of V are obtained. Report your answers to the correct number of significant figures.
8. A 2.856-g sample of limestone was analyzed for Fe, Ca, and Mg. The iron was determined as Fe;Os, yielding 0.04561 g. Calcium was isolated as CaSO4, yielding a precipitate of 1.487 g, and Mg was isolated as 0.1599 g of Mg;P2O7. Report the amount of Fe, Ca, and Mg in the limestone sample as %w/w FeO, %w/w CaO, and %w/w MgO.
Calculate the volume (in L) of Carbon dioxide that will be formed if 25.0 grams of potassium oxalate will react with potassium permanganate in the solution. The density of the carbon dioxide is 1.98 kg/m3 K2C2O4 + KMnO4 + H2O ----> CO2 + Mn (OH)2 + KOH (Molar mass: Potassium hydroxide: 56.11 g/mol; Potassium permanganate: 158.04 g/mol; Water: 18 g/mol; Carbon dioxide: 44 g/mol; Potassium oxalate: 166.20 g/mol; Manganese (II) hydroxide: 88.96 g/mol)
A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.
A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O. a.Write the ionic equation for the reaction. b.Write the net ionic equation for the reaction. c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture? d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture? e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)? f.What is the percent by mass of each salt in the mixture
Balance the following equation. If the coefficient is "1," you must enter the 1. C2H5NH2(1) + 02(g) --> CO2(g) + H20(1) + N2(g)
(A). List one of the Products in the following unbalanced chemical reaction: C₆H₁₂O₆ + O₂ --> H₂O + CO₂ (B). When you balance the above equation the coefficients are 1:6:__:6 find the blank to balance the Hydrogens.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS