Please i have question:
When we prepared nitrate of cerium (Ce(NO3)3) based on CeO2 oxide, why the amount of nitric acid is non stochiometric which it should be with excess in the chemical equation?
Thank you
Not clear to me why you start with CeO2 - the oxide of Ce(4+) - and hope to obtain the nitrate of Ce(3+). Nitric acid will not reduce Ce(4+) to Ce(3+). You would need a reducing agent in the mixture, but one mild enough not to be oxidized by nitric acid - a significant complication, and in my opinion unnecessary.
I would recommend starting with Ce(OH)3 or with the carbonate, Ce2(CO3)3 instead of CeO2.
Thank you, dear sir for your response
This reaction is done in two parts:
Part 1: To form Ce2O3 with the chemical equation:
2 Ce2O3 + 3O2 --------- 4CeO2
Part 2: To form (Ce(NO3)3) with the chemical equation:
Ce2O3+6HNO3---------- 2Ce(NO3)3+ 3H2O
unfortunately, we don't have directly the product Ce2O3 to do it
Can you make any suggestion for this case?
Thank you
With best regards..
Some additional references that you may want to look at:
Article Reduction Mechanism for CeO 2 Revealed by Direct Observation...
In Situ Oxidation and Reduction of Cerium Dioxide Nanoparticles Studied by Scanning Transmission Electron Microscopy / Aaron C. Johnston-Peck* , †, Wei-Chang D. Yang‡ , #, Jonathan P. Winterstein‡, Renu Sharma‡, and Andrew A. Herzing* , † (NIST report available free of charge)
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