13.73 What is its molarity after a reaction time of 5.00 days? Express your answ

Question

13.73

What is its molarity after a reaction time of 5.00 days? Express your answer using two significant figures Constants | Periodic Table Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI and the rate constant is 9.7 × 10-6M-1 s-1. If the initial concentration of HI is 0.110 M [HI] = Submit Request Answer Part B What is the time (in days) when the HI concentration reaches a value of 7.5x10-2 M Express your answer using two significant figures days Submit Request Answer Provide Feedback Next>

Explanation / Answer

For a second order reaction (1/A) = (1/Ao)+ kt
Where
Ao = initial concentration = 0.110 M
A = concentration left after time t = ?
t = time taken = 5.00 days*(24 hr/ day)*(60 min/ hr)*(60 s/ min)= 432*10^3 s
k = rate constant = 9.7*10^-6 M^-1s^-1
Plug the values we get
(1/A) = (1/Ao) +kt
= 13.3
A = 0.075 M
Therefore the concentration of HI after 5 days is 0.075M

Part B:

In the similar manner as done above when A= 7.5*10^-2M

time taken,t= 437.4*10^3 s*(1 min/ 60 s)*(1 hr/60 min)*(1 day/24hr)= 5.0 days

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