From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 5.600 g Mass of FeCl3 : 1.60 g From Part B: % Potassium in compound : 23.23 % % Iron (from ion exchange & titration vs. NaOH) : 8.25 % From Part C: % Oxlate : 56.78 % Calculate the following for C2O42-: g in 100 g sample mol in 100 g sample mol/mol Fe (3 sig figs) mol/mol Fe (whole number)

From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 5.600 g Mass of FeCl3 : 1.60 g From Part B: % Potassium in compound : 23.23 % % Iron (from ion exchange & titration vs. NaOH) : 8.25 % From Part C: % Oxlate : 56.78 % Calculate the following for C2O42-: g in 100 g sample mol in 100 g sample mol/mol Fe (3 sig figs) mol/mol Fe (whole number)

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

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

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

Chapter21: The Chemistry Of The Main Group Elements

Section: Chapter Questions

Problem 86GQ: In 1774, C. Scheele obtained a gas by reacting pyrolusite (MnO2) with sulfuric acid. The gas, which...

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

From Part A:

Mass of K_xFe(C₂O₄)_y · zH₂O prepared : 5.600 g
Mass of FeCl₃ : 1.60 g

From Part B:

% Potassium in compound : 23.23 %
% Iron (from ion exchange & titration vs. NaOH) : 8.25 %

From Part C:

% Oxlate : 56.78 %

Calculate the following for C₂O₄^2-:

g in 100 g sample

mol in 100 g sample

mol/mol Fe
(3 sig figs)

mol/mol Fe
(whole number)

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