The following mechanism for the gas phase reaction of H_2 and ICI that is consis
ID: 1006379 • Letter: T
Question
The following mechanism for the gas phase reaction of H_2 and ICI that is consistent with the observed rate law is: step 1 slow: H_2(g) + ICI(g) rightarrow HCl(g) + HI(g) step 2 fast: ICI(g) + HI(g) rightarrow HCl(g) + I_2(g) What is the equation for the overall reaction? Use the smallest integer coefficients possible If a box is not needed, leave it Blank. 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: Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]^m[B]^n..., where "1" is understood (so don't write it) for m, n etc. Rate =Explanation / Answer
Given steps :
Step-1: Slow H2 (g) + ICl (g) --------------> HCl (g) + HI (g)
Step-2) Fast: ICl (g) + HI (g) ------------------> HCl (g) + I2 (g)
1) For Net reaction let us add these two reactions,
H2 (g) + 2 ICl (g) + + HI (g) --------------> 2 HCl (g) + HI (g) + I2 (g)
HI (g) is common on both sides and hence get cancelled out mutually and hence we get,
H2 (g) + 2 ICl (g) + --------------> 2 HCl (g) + I2 (g)
2) Catalyst is the species that participate in the reaction but finally recovered back unchanged or original form.
Both reactants i.e. H2 (g) and ICl (g) consumed in the reaction and not generated back so
No species act as a catalyst.
3) Intermediate : Is the species in the reaction which has transitory existance and get decomposed into the product(s).
An intermediate may or may not be isolable but certainly do not exist for long and eventually breaks into the product.
In given reaction we can see the species HI (g) which forms in step-1 but eventually decomposed by ICl (g) into the the products HCl (g) and I2 (g)
Hence HI (g) is a reaction Intermediate.
4) Overall reaction is,
H2 (g) + 2 ICl (g) + --------------> 2 HCl (g) + I2 (g)
Hence rate law for this reaction is,
In rate law the concentration of each reactant raised to the power equal to stoichiometric coefficient of that species in reaction equation.
Rate = k [ICl]2[H2]1
Rate = k [ICl]2[H2].
Where k is rate constant.
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