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Sonja [21]
3 years ago
11

Iron in the 2 oxidation state reacts with potassium dichromate to produce Fe3 and Cr3 according to the equation: 6 Fe2 (aq) Cr2O

72-(aq) 14 H (aq) <----> 6 Fe3 (aq) 2 Cr3 (aq) 7 H2O(l) How many milliliters of 0.2937 M K2Cr2O7 are required to titrate 132.0 mL of 0.1782 M Fe2 solution
Chemistry
1 answer:
allsm [11]3 years ago
6 0

Given :

Volume of Fe^{2+} , V = 132 mL .

Molarity of Fe^{2+}, M = 0.1782 M .

To Find :

How many milliliters of 0.2937 M K_2Cr_2O_7 are required to titrate 132.0 mL of 0.1782 M Fe^{2+} solution .

Solution :

Moles of  Fe_2 :

n=0.1782\times \dfrac{132}{1000}\ mol\\\\n=0.264\ mol

Now , 1 mole of K_2Cr_2O_7 reacts with 6 mole of Fe^{2+} .

So , moles of K_2Cr_2O_7 required is :

N=\dfrac{0.264}{6}=0.044\ mol

Volume required is :

V=\dfrac{N}{M}\\\\V=\dfrac{0.044}{0.2937}\ L\\\\V=0.15\ L=150\ mL

Hence , this is the required solution .

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To determine the enthalpy and entropy of dissolving a compound, you need to measure the Ksp at multiple temperatures. Then, plot ln(Ksp) vs. 1/T. The slope of the plotted line relates to the enthalpy (ΔH) of dissolving and the intercept of the plotted line relates to the entropy (ΔS) of dissolving.

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us use the thermodynamic definition of the Gibbs free energy and its relationship with Ksp as follows:

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Thus, by combining them, we obtain:

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y=mx+b

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It means that we answer to the blanks as follows:

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Regards!

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