Cl2(g) ↔ 2Cl(g)
Cl(g) + CHCl3 → HCl(g) + CCl3 (slow)
CCl3 + Cl(g) → CCl4(g) (fast)
Which of the following are true statements for the above mechanism ?
a) Cl(g) does not appear directly in the overall rate law
b) k1[Cl2] = k-12[Cl]
c) Cl(g) does not appear in the overall reaction
d) If this is a correct mechanism the observed law would be
Rate = k[Cl2]1/2[CHCl3]
2007-02-06 16:34:05 · 1 answers · asked by Hasan S 1 in Science & Mathematics ➔ Chemistry
The overall reaction is Cl2 + CHCl3 -> HCl +CCl4 so
the overall reaction rate is K=[Cl2][CHCl3]/[HCl][CCl4] so (a.) is false.
The first reaction at equilibrium must have the same rate forward as backwards so k1[Cl2]=k^-1[Cl]^2 so (b.) is false.
The overall does not have Cl so (c.) is true and (d.) is false.
2007-02-09 15:39:26 · answer #1 · answered by LGuard332 2 · 0⤊ 0⤋