Question

At a certain temperature the rate of this reaction is first order in HI with a rate constant of :7.21/s2HI(g) = H2(g) + I2(g)Suppose a vessel contains HI at a concentration of 0.440M. Calculate the concentration of HI in the vessel 0.210 seconds later. You may assume no other reaction is important.

Answer 1

C HI = 0.0968 M

Step-by-step explanation:

• 2HI(g) → H2(g) + I2(g)
• - ra = K(Ca)∧α = - δCa/δt

∴ a: HI(g)

∴ order (α) = 1

∴ rate constant (K) = 7.21/s

∴ Initial concenttration HI(g) (Cao) = 0.440 M

∴ t = 0.210 s ⇒ Ca = ?

⇒ - δCa/δt = KCa

⇒ - ∫δCa/Ca = K*∫δt

⇒ Ln(Cao/Ca) = K*t

⇒ Cao/Ca = e∧(K*t)

⇒ Cao/e∧(K*t) = Ca

⇒ Ca = (0.440)/e∧((7.21*0,21))

⇒ Ca = 0.440/4.54533

⇒ Ca = 0.0968 M