Please help me with this one...
What is the oxidizing agent in the following redox reaction:
HNO3(aq) + K2CrO4(aq) + Fe(NO3)2(aq) ->
KNO3(aq) + Fe(NO3)3(aq) + Cr(NO3)3(aq) + H2O(l)
?
First one: Cr starts at +6 each and ends at +3. Fe(II) starts at +2 and ends at +3.
Oxidation is the loss of electrons.
Yea so it would be K2CrO4
To determine the oxidizing agent in a redox reaction, we need to identify which species is undergoing reduction. The species that is being reduced is the oxidizing agent.
In the given reaction, we can assign oxidation states to each element:
HNO3(aq): In this compound, hydrogen (H) has an oxidation state of +1, nitrogen (N) has an oxidation state of +5, and oxygen (O) has an oxidation state of -2.
K2CrO4(aq): In this compound, potassium (K) has an oxidation state of +1, chromium (Cr) has an oxidation state of +6, and oxygen (O) has an oxidation state of -2.
Fe(NO3)2(aq): In this compound, iron (Fe) has an oxidation state of +2, nitrogen (N) has an oxidation state of +5, and oxygen (O) has an oxidation state of -2.
KNO3(aq): In this compound, potassium (K) has an oxidation state of +1, nitrogen (N) has an oxidation state of +5, and oxygen (O) has an oxidation state of -2.
Fe(NO3)3(aq): In this compound, iron (Fe) has an oxidation state of +3, nitrogen (N) has an oxidation state of +5, and oxygen (O) has an oxidation state of -2.
Cr(NO3)3(aq): In this compound, chromium (Cr) has an oxidation state of +3, nitrogen (N) has an oxidation state of +5, and oxygen (O) has an oxidation state of -2.
H2O(l): In this compound, hydrogen (H) has an oxidation state of +1, and oxygen (O) has an oxidation state of -2.
From the given reaction, we can see that the oxidation state of chromium in K2CrO4(aq) is reduced from +6 to +3 in Cr(NO3)3(aq). Therefore, chromium is being reduced and is the oxidizing agent in this redox reaction.
So, the oxidizing agent is Cr(NO3)3(aq) (chromium nitrate).