Ch.18 - ElectrochemistryWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Chromium can be electroplated from an aqueous solution containing sulfuric acid and chromic acid, H2CrO4. What current (A) is required to deposit chromium at a rate of 1.25 g/min? Enter your answer as the nearest whole number and no units.

Problem

Chromium can be electroplated from an aqueous solution containing sulfuric acid and chromic acid, H2CrO4. What current (A) is required to deposit chromium at a rate of 1.25 g/min? Enter your answer as the nearest whole number and no units.

Solution

We’re being asked to calculate current (A) is required to deposit chromium at a rate of 1.25 g/min.


We can now calculate the mass of Cr(s) deposited.

Step 1: Calculate the charge of chromium from H2CrO4.
Step 2: Calculate the mole Chromium used.
Step 3
: Calculate the Calculate mole electrons used.
Step 4: Calculate the Current.


Step 1Calculate the charge of chromium from H2CrO4.

H → Group 1A → +1 charge

O → Not on a peroxide or superoxide → -2 charge


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