A 13.2010g sample of hydrated zinc sulfate, ZnSO4 • xH2O), was strongly heated until no further change in mass was recorded. The final mass of solid product was found to be 7.3997g. On heating, all of the water of crystallization had evaportaed, as shown by the equation: ZnSO4 • xH2O -> ZnSO4 + xH2O  Calculate the number of moles of water of crystallization in the sample. Write in a padpaper and show the complete solution

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A: Molarity = moles ÷ volume (L)  Mole = molarity × volume (L)  Mass = mole × molar mass

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A:

Q: エ

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A: This is the concept of Organic chemistry

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A: Question 2

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Q: deltaG

A:

Q: activity 1. Problem Solving Directions: Calculate the AS for each given reaction. Show your complete...

A: Change in entropy ΔS0 for a reaction is given by,      ΔS0rxn  = Σ S0products - Σ S0reactants