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If 60.13g of Nb(s) are added to 125.0ml of a 5.96mL of a 5.96 M solution of HClO4(aq), what is the mass of Nb(ClO4)5(aq) that is produced?

If 60.13g of Nb(s) are added to 125.0ml of a 5.96mL of a 5.96 M solution of HClO4(aq), what is the mass of Nb(ClO4)5(aq) that is produced?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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If 60.13g of Nb(s) are added to 125.0ml of a 5.96mL of a 5.96 M solution of HClO4(aq), what is the mass of Nb(ClO4)5(aq) that is produced?

Expert Solution
Step 1

Given that - 

Mass of Nb(s) = 60.13 g 

Volume of HClO4 Solution = 125.0 mL 

Molarity of HClO4 Solution = 5.96 M 

 

The Balanced Chemical equation between HClO4 and Nb is - 

 

10HClO4(aq) + 2Nb(s) ------> 2Nb(ClO4)5(aq) + 5H2 

 

The molar masses of substances are - 

HClO4 = 100.46 g/mol

Nb = 92.906 g/mol

Nb(ClO4)5 = 590.159 g/mol

 

According to this reaction , 10×100.46 g or 10 moles of HClO4 react with 2×92.906 g or 2 moles of Nb to give 2 moles or 2×590.159 g Nb(ClO4)5

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