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At standard conditions, solutions of hydrogen peroxide, H2O2, iron(III) nitrate, Fe(NO3)3, and iron(II) nitrate, Fe(NO2)2, were added to a beaker - VCE - SSCE Chemistry - Question 30 - 2023 - Paper 1
Question 30
At standard conditions, solutions of hydrogen peroxide, H2O2, iron(III) nitrate, Fe(NO3)3, and iron(II) nitrate, Fe(NO2)2, were added to a beaker. The initial concen... show full transcript
Worked Solution & Example Answer:At standard conditions, solutions of hydrogen peroxide, H2O2, iron(III) nitrate, Fe(NO3)3, and iron(II) nitrate, Fe(NO2)2, were added to a beaker - VCE - SSCE Chemistry - Question 30 - 2023 - Paper 1
Step 1
C. The concentration of H2O2(aq) decreases immediately since it is the strongest reducing agent.
Answer
In this scenario, hydrogen peroxide (H2O2) acts as a strong oxidizing agent with potential to undergo decomposition reactions. Because it is more thermodynamically favorable for H2O2 to reduce, its concentration will decrease swiftly as it reacts with the available iron ions in solution.
The reaction typically involves the oxidation of iron(II) ions to iron(III), facilitated by the H2O2. Given that H2O2 is a stronger reducing agent in these conditions, its consumption is immediate, confirming that statement C is correct.