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Question
Which of the following graphs is correct for a first order reaction?
Solution
Explanation:
The pace of a reaction that is directly proportional to the concentration of the reacting substance is known as a first-order reaction.
A first-order reaction's kinetic equation
k = `2.303/t log [R]^0/([R])`
The Y-axis represents concentration, whereas the X-axis represents time.
`log = [R]^0/([R]) = (kt)/2.303`
`[log = [R]_0/([R])] = [(kt)/2.303](t)`
y = mn
k = `2.303/t log a/(a - x)`
t = `2.303/k log a/(a - x)`
x = `a - a/2`
x = `a/2`
`t_(1/2) = 2.303/k log a/(a - a/2)`
`2.303/k log 2`
`t_(1/2) = 0.693/k`
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