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 H2O 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 H2O g in 100 g sample mol in 100 g sample mol/mol Fe (3 sig figs) mol/mol Fe (whole number)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 72QRT

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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 H₂O

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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