What Are Three Uses of Rhodium as a Catalyst?

  • Thread starter Thread starter Physics345
  • Start date Start date
  • Tags Tags
    Catalyst
Click For Summary
SUMMARY

Rhodium serves as a catalyst in three significant chemical reactions: the reduction of nitrogen oxides, the carbonylation of methanol, and the vapor conversion of carbon monoxide to carbon dioxide. The balanced equations for these reactions are as follows: for nitrogen oxides, 2NO_x → xO_2 + N_2; for carbonylation, H3COH + CO → H3CCOOH. However, the vapor conversion reaction CO + H2O → CO2 + H+ is technically impossible to balance, indicating that the proposed reaction must be revised for accuracy.

PREREQUISITES
  • Understanding of chemical reactions and catalysts
  • Familiarity with balanced chemical equations
  • Knowledge of nitrogen oxides and carbon monoxide chemistry
  • Basic principles of carbonylation reactions
NEXT STEPS
  • Research the principles of catalytic reactions in organic chemistry
  • Study the mechanisms of nitrogen oxide reduction
  • Learn about carbonylation processes and their applications
  • Examine the limitations of reaction equations in catalysis
USEFUL FOR

Chemistry students, chemical engineers, and professionals involved in catalysis research will benefit from this discussion, particularly those focusing on environmental chemistry and industrial applications of catalysts.

Physics345
Messages
250
Reaction score
23

Homework Statement


I was reviewing chem the other day, and noticed this question can anyone clarify my answer for me and let me know if I'm correct.

The question states:

Describe three uses of rhodium as a catalyst. ( include both a written description and the balancecd equation).

Homework Equations

The Attempt at a Solution


[/B]
The rhodium in this case will help catalyze the reduction of nitrogen oxides [2NO_x → xO_2+N_2]. Secondly another use would be of the carbonylation reaction by adding a carbon dioxide molecule into methanol. H_3 COH+CO→H_3 CCOOH. Thirdly and finally, it can be used as vapour conversion of carbon oxide to carbon dioxide, which reduces water by adding a carbon dioxide molecule which looks like this: CO+H_2 O→CO_2+H^+
 
Physics news on Phys.org
The last reaction - as written - is technically impossible (can't be balanced).
 
  • Like
Likes   Reactions: Physics345
Borek said:
The last reaction - as written - is technically impossible (can't be balanced).
Hi Borek, it's been a while! First off thanks for the reply it is very much appreciated.
But there is vapour conversion of carbon oxide to carbon dioxide right?
Also why exactly is it impossible?
 
Last edited:
You can't balance the equation, so the process can't follow it.

Doesn't mean there is no vapor conversion of oxides, just the reaction equation must be different.
 
  • Like
Likes   Reactions: Physics345
Borek said:
You can't balance the equation, so the process can't follow it.

Doesn't mean there is no vapor conversion of oxides, just the reaction equation must be different.
CO2 + OH ---> CO + H2O
Would it look more like this then?
 
No such thing as OH (unless you mean a hydroxyl radical, but radicals are so reactive they don't need a catalyst).

Plus, it still can't be balanced.
 
  • Like
Likes   Reactions: Physics345
Borek said:
No such thing as OH (unless you mean a hydroxyl radical, but radicals are so reactive they don't need a catalyst).

Plus, it still can't be balanced.
What exactly am I not understanding here?
Also is there any thing I should relearn to understand this better?
 
Catalyst can work only on real reactions - that means a balanced equation. Try to balance the two equations you posted.
 

Similar threads

Chemically regenerating my auto's catalytic converter?
  • · Replies 19 ·
Replies
19
Views
8K
Rising Carbon Dioxide Levels Don’t Increase Earth’s Temperature
  • · Replies 28 ·
Replies
28
Views
28K