   Chapter 20, Problem 21E

Chapter
Section
Textbook Problem

# What mass of barium is produced when molten BaCl2 is electrolyzed by a current of 2.50 × 105 A for 6.00 h?

Interpretation Introduction

Interpretation: The current required and the time taken for the electrolysis of BaCl2 is given. The mass of barium produced is to be calculated.

Concept introduction: The process of decomposition of compounds by passing electricity through a solution is known as electrolysis.

To determine: The mass of barium produced after the electrolysis of BaCl2 .

Explanation

Explanation

Given

Current passed during electrolysis is 2.50×105A .

Time of electrolysis is 6.00h .

The atomic mass of barium is 137.3g .

The reaction that takes place during the electrolysis of BaCl2 is,

Ba2+(aq)+2eBa(s)

The conversion of hours (hr) into seconds (s) is done as,

1hr=3600s

Hence,

The conversion of 6hr into seconds is,

6hr=(6×3600)s=21600s

The conversion of second (s) into Coulombs per second (C/s) is done as,

1s=2.5×105C/s

Hence,

The conversion of 21600s into Coulombs per second is,

21600s=(21600×2.5×105)C/s=5.4×109C/s

The conversion of Coulombs per second (C/s) into Coulombs per mole is done as,

1C/s=196485Cmol

Hence,

The conversion of 5

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