Iodine atoms combine to form molecular iodine in the gas phase: I_(g) + I_(g) ri

Question

Iodine atoms combine to form molecular iodine in the gas phase: I_(g) + I_(g) righarrow I_2(g) This reaction has a rate constant of 7.0 times 10^9 M^-1 S^-1 at 23 degree C. If the initial concentration of I is 0.086M, calculate the concentration after 2.0 minutes. Also, calculate the concentration after 2.0 minutes. Also, calculate the half-life for this reaction. This is a second-order rate constant. Use the integrated rate law for a second-order reaction: 1/[1]_t = kt + 1/[1]_0 = (7.0x10^9 M^-1 S^-1)(120s)+1/0.086M = 8.4x10^11M^-1 [I]_t = 1/8.4x10^11M^-1 = 1.2x10^-2 M

Explanation / Answer

k2 = x/t(a-x)a

7*10^9 = (x/(2*60*(0.086-x)*0.086))

x = 0.086 M

t1/2 = ((0.086/2)/(7*10^9*(0.0862/2)*0.086))

     = 1.65*10^(-9) sec

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