The following mechanism for the gas phase reaction of H2 and ICI that is consist
ID: 705039 • Letter: T
Question
The following mechanism for the gas phase reaction of H2 and ICI that is consistent with the observed rate law is: step 1 slow: H2(g) + Cl(g)-? HCI(g) + HI(g) step 2 fast: ICl(g)+ HI(g) HCIg) 12(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 omplete the rate law for the overall reaction that is consistent with this mechanism. (Use the form kIAl" BI".., where 'I' is understood (so don't write it) for m, n etc.) Rate Retry Entire Group 9 more group attempts remaining NextExplanation / Answer
Answer - Part 1.
The balanced overall reaction is -
H2(g) + 2 ICl(I) ---> 2 HCl(g) + I2(g)
Our mechanism suggests that HI is consumed in the second step as fast as it is being formed. HI is, therefore, the reaction intermediate.
The HI not include in overall reaction hence HI(g) is reaction intermidate
The rate = k[ICl][H2]
None of the species act as a catalyst.
Part -2
The balanced chemical reaction is-
NO(g) + O3(g) -> NO2(g) + O2(g)
Rate = k [NO] [O3]
NO2 is reaction intermidate beacause as it produced in reaction 1 consumed in reaction 2.
O is catalyst.
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