AH for the reaction IF5 (g) → IF3 (g) + F2 (g)

kJ, give the data below.

IF (8) + F2 (g) → IF3 (8)

IF (g) + 2F2(8) ► F5 (8)

AH=-390 kJ

AH=-745 kJ

A) -1135

B) +35

C) +1135

D) -35

E) +355

At a certain temperature the rate of this reaction is first order in hi with a rate constant of : 0.0632s2hig=h2g+i2g suppose a vessel contains hi at a concentration of 1.28m . calculate how long it takes for the concentration of hi to decrease to 17.0% of its initial value. you may assume no other reaction is important. round your answer to 2 significant digits.