The following mechanism for the gas phase reaction of H2 and ICl that is consist
ID: 501319 • Letter: T
Question
The following mechanism for the gas phase reaction of H2 and ICl that is consistent with the observed rate law is: step 1 slow: H2(g) Ici(g) e HCl (g) HI(g) step 2 fast ICI(g) HI(g) HCl(g) (g) (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 (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form klAlmIB] where 'l' is understood (so don't write it for m, n etc.) RateExplanation / Answer
1,The reactions are H2(g) + ICl(g) -----à HCl (g) + HI(g)
ICl(g) + HI(g) ------àHCl(g) + I2(g)
Subtracting the two reaction gives H2-HI ------ HI-I2
Or H2(g)+I2(g)-----à2HI, Overall reactions
There are two intermediates, HCl and ICl and there is no catalyst.
Slow reaction determies the rate of reaction. Accordingly , rate= K[H2] [ICL], K is rate constant.
2. The reactions are O3+NO-àNO2+ O2 and NO2+O--àNO + O2
Addition of the two reactions gives O3+O--à2O2(g)
Nascent oxygen acts as a catalyst. NO and NO2 are intermediates.
Rate law , r = K[O3][NO]
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.