Problem: Consider the unbalanced redox reaction:Cr2O72–(aq) + Cu(s) → Cr 3+ (aq) + Cu 2+(aq)Balance the equation and determine the volume of a 0.850 M K2Cr2O7 solution required to completely react with 5.25 g of Cu. 

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We are being asked to determine the volume of K2Cr2O7 solution to completely react with 5.25 g of Cu. We will calculate the amount of K2Cr2O7 using the balanced redox reaction equation and mol to mol comparison.


Let’s balance the redox reaction first. We will assume that the reaction is under acidic condition unless stated otherwise. When balancing redox reactions under acidic conditions, we will follow the following steps.


Step 1: Separate the whole reaction into two half-reactions

Step 2: Balance the non-hydrogen and non-oxygen elements first

Step 3: Balance oxygen by adding H2O to the side that needs oxygen (1 O: 1 H2O)

Step 4: Balance hydrogen by adding H+ to the side that needs hydrogen (1 H: 1 H+)

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Problem Details

Consider the unbalanced redox reaction:
Cr2O72–(aq) + Cu(s) → Cr 3+ (aq) + Cu 2+(aq)
Balance the equation and determine the volume of a 0.850 M K2Cr2O7 solution required to completely react with 5.25 g of Cu.

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Our tutors have indicated that to solve this problem you will need to apply the Balancing Redox Reactions: Acidic Solutions concept. You can view video lessons to learn Balancing Redox Reactions: Acidic Solutions. Or if you need more Balancing Redox Reactions: Acidic Solutions practice, you can also practice Balancing Redox Reactions: Acidic Solutions practice problems.

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

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Our data indicates that this problem or a close variation was asked in Chemistry: A Molecular Approach - Tro 3rd Edition. You can also practice Chemistry: A Molecular Approach - Tro 3rd Edition practice problems.