1. Consider the following reactionI205(9) + 5 CO)→ 5 CO2(9) + 12(9)a. If 80.0 grams of iodine(V) oxide, IO5, reacts with 28.0 grams of carbon monoxide, COdetermine the mass of I2 that can be produced. (theoretical)b. If, in the above situation, only 0.160 moles, of iodine, I2@ was produced.What mass of iodine was produced? (actual)ii. What is the percentage yield of iodine for this reaction?i.

We will calculate all the parts

30.0 grams of iodine(V) oxide, I½O5, reacts with 28.0 grams of carbon monoxide, cermine the mass of I2 that can be produced. (theoretical) in the above situation, only 0.160 moles, of iodine, I2@ was produced. What mass of iodine was produced? (actual) What is the percentage yield of iodine for this reaction?

30.0 grams of iodine(V) oxide, I½O5, reacts with 28.0 grams of carbon monoxide, cermine the mass of I2 that can be produced. (theoretical) in the above situation, only 0.160 moles, of iodine, I2@ was produced. What mass of iodine was produced? (actual) What is the percentage yield of iodine for this reaction?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

Problem 3.87PAE: 3.87 Nitric acid (HNO3) can be produced by the reaction of ni- trogen dioxide (NO2) and water....

See similar textbooks

Similar questions

Chlorine exists mainly as two isotopes, 37Cl and 33Cl. Which is more abundant? How do you know?
The compound As2I4 is synthesized by reaction of arsenic metal with arsenic triiodide. If a solid cubic block of arsenic (d = 5.72 g/cm3) that is 3.00 cm on edge is allowed to react with 1.01 1024 molecules of arsenic triiodide, what mass of As2I4 can be prepared? If the percent yield of As2I4 was 75.6%, what mass of As2I4 was actually isolated?
Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane: 2NH3(g)+3O2(g)+2CH4(g)2HCN(g)+6H2O(g) If 5.00 103 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H2O will be produced, assuming 100% yield?
4.104 When 2.750 g of the oxide Pb3O4 is heated to a high temperature, it decomposes to produce 0.0640 g of oxygen gas and 2.686 g of some new lead oxide compound. How can you use these data to determine the formula of the new compound?
4.80 The reaction shown below is used to destroy Freon-12 (CF2Cl2), preventing its release into the atmosphere. What mass of NaF will be formed if 250.0 kg of CF2Cl2 and 400.0 kg of Na2C2O4 are heated and allowed to react to completion? CF2Cl2+2Na2C2O42NaF+2NaCl+C+4CO2
Copper metal reacts with mine acid. Assume that the reaction is 3Cu(s)+8HNO3(aq)3Cu(NO3)2(aq)+2NO(g)+4H2O(l) If 5.58 g Cu(NO3)2 is eventually obtained, how many grams of nitrogen monoxide, NO, would have formed?
3.87 Nitric acid (HNO3) can be produced by the reaction of ni- trogen dioxide (NO2) and water. Nitric oxide (NO) is also formed as a product. Write a balanced chemical equation for this reaction.
The deep blue compound Cu(NH3)4S04 is made by the reaction of copper(II) sulfate and ammonia CuSO4(aq) + 4 NH3(aq) Cu(NH3)4SO4(aq) (a) If you use 10.0 g of CuSO4 and excess NH3, what is the theoretical yield of Cu(NH3)4SO4? (b) If you isolate 12.6 g of Cu(NH3)4SO4, what is the percent yield of Cu(NH3)4SO4?
A mixture of Fe2O3, and FeO was found to contain 72.00% Fe by mass. What is the mass of Fe2O3 in 0.750 g of this mixture?