# 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

100% (1 ratings) ###### 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.