Use the References to access important values if needed for this question. The f
ID: 718121 • Letter: U
Question
Use the References to access important values if needed for this question. The following is a proposed mechanism for the gas phase decomposition of nitryl chloride. step 1 fast: NO2CNO2+CI step 2 slow: NO2CI+ CNO2+ Ch (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank Which species acts as a reaction intermediate? Enter formula. If none, leave box blank (3) (4) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A][B]n-where '1, is understood (so don't write it if it's a "I') for m, n etc. Rate-Explanation / Answer
Ans 1
To get the Overall equation add the two reactions
2 NO2Cl - - - - > 2 NO2 + Cl2
Ans 2
There is no catalyst used in this reaction. Catalyst is represented as a reactant and end up in the product.
Ans 3
In the first reaction Cl is produced and in the second reaction Cl is consumed, therefore, Cl acts as a reaction intermediate.
Ans 4
Rate law for the overall reaction
Rate = k [NO2Cl]2
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