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.

FREE Expert 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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Problem Details

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.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Electroplating concept. If you need more Electroplating practice, you can also practice Electroplating practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Daly's class at ARIZONA.