The correct option is B (NH4)2Cr2O7Δ→N2+Cr2O3+3H2O
Analysing the options
Option (A)
2CrO2−4+2H+→Cr2O2−7+H2O
Let oxidation state of Cr in CrO2−4=x
x+4(−2)=−2
⇒x−8=−2
∴x=+6
Let oxidation state of Cr in Cr2O2−7=x
2x+7(−2)=−2
⇒2x−14=−2
∴x=+6
In this reaction, oxidation no. of Cr is +6 in both CrO2−4 and Cr2O2−7.
Option (B)
Cr2O2−7+2OH−→2Cr2O2−4+H2O
In this reaction also, oxidation no. of Cr is +6 in both CrO2−4 and Cr2O2−7.
Option (C)
CrO2Cl2+2OH−→CrO2−4+2HCl
Oxidation state Cr in CrO2Cl2 be x
x+2(−2)+2(−1)=0
⇒x−6=0
∴x=+6
Oxidation state of Cr in (CrO2−4) is 6 (as calculated)
x+4(−2)=−2
⇒x−8=−2
∴x=+6
In this reaction , oxidation no. of Cr is +6 in both CrO2Cl2 and CrO2−4.
Option (D)
(NH4)2Cr2O7Δ→N2+Cr2O3+3H2O
Oxidation state : Cr in Cr2O2−7=+6
Oxidation number of Cr in Cr2O3=+3
The oxidation no. of Cr thus decreases from +6 to +3 in this reaction.
So, the correct answer is option (D).