1)81.2g,57.8g,101.1g,334.7g,124.5g,or 23.22)the second picture In the chemical engineering lab last weecomplete decomposition of 435.8 g ofammonium dichromate (molar mass == 25g/mol) produced 101.1 g H20.(NH4)2C12O7(s)Cr2O3(s) + N211 What ic the thonrntical viold of waterV [ Select ]|81.2%ateLess than 10%40.1%18.2%57.8%More than 100%23.2%r (Aextracted from ores of AgK(CN)2 (potassA In the chemical engineering lab last week, thecomplete decomposition of 435.8 g ofammonium dichromate (molar mass = 252.1g/mol) produced 101.1 g H20.(NH4)2C12O7(s) -Cr2O3(s) + N2(g) + 4H1) What is the theoretical yield of waterproduced? [ Select ]2) Determine the percent yield for water.[ Select ]<>

Answered: Image /qna-images/answer/ad8fb43b-9ab7-434e-949d-c54037e9e969.jpg

In the chemical engineering lab last week, the complete decomposition of 435.8 g of ammonium dichromate (molar mass = 252.1 g/mol) produced 101.1 g H20. (NH4)2C12O7(s) → Cr2O3(s) + N2(g) + 4F 1) What is the theoretical yield of water produced? [ Select ] 2) Determine the percent yield for water. [ Select ] <>

In the chemical engineering lab last week, the complete decomposition of 435.8 g of ammonium dichromate (molar mass = 252.1 g/mol) produced 101.1 g H20. (NH4)2C12O7(s) → Cr2O3(s) + N2(g) + 4F 1) What is the theoretical yield of water produced? [ Select ] 2) Determine the percent yield for water. [ Select ] <>

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter12: Gravimetric Methods Of Analysis

Section: Chapter Questions

Problem 12.19QAP

See similar textbooks

Similar questions

Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker containing 20.0 g of NaOH. Not all the NaOH was consumed. How many grams of NaOH were left unreacted? The equation for the reaction is H3PO4(aq)+3OH(aq)3H2O+PO43(aq)
The metals industry was a major source of air pollution years ago. One common process involved roasting metal sulfides in the air 2 PbS(s) + 3 O2(g) 2 PbO(s) + 2 SO2(g) If 2.50 mol of PbS is heated in air, what amount of O2 is required for complete reaction? What amounts of PbO and SO2 are expected?
Small quantities of oxygen gas can be generated in the laboratory by the decomposition of hydrogen peroxide. The unbalanced equation for the reaction is H2O2(uz/)-? H2O(/) + O2(g) Calculate the mass of oxygen produced when 10.00 g of hydrogen peroxide decomposes.
Hexamethylenediamine (C6H16N2) is one of the starting materials for the production of nylon. It can be prepared from adipic acid (C6H10O4) by the following overall equation: C6H10O4(l) + 2NH3(g) + 4H2(g) C6H16N2 (l) + 4H2O (l) What is the percent yield for the reaction if 765 g of hexamethylenediamine is made from 1.00 103 g of adipic acid?
The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
How many molecules of the sweetener saccharin can be prepared from 30 C atoms, 25 H atoms, 12 0 atoms, 8 S atoms, and 14 N atoms?