Question

In: Chemistry

In The first order reaction A -> products, [A] = .400 M initally and .250 M...

In The first order reaction A -> products, [A] = .400 M initally and .250 M after 15 min, what will [A] be after 175 min?

Expert Solution

Calculation of rate constant :

For a first order reaction rate constant , k = ( 2.303 /t )x log ( M_o / M)

Where

M_o = initial concentration = 0.400 M

M = concentration after time t = 0.250 M

t = time = 15 min

k = rate constant = ?

Plug the values we get k = ( 2.303 /15 )x log (0.400 / 0.250)

= 0.0313 min^-1

Now calculation of concentration of A after 175 min :

For a first order reaction rate constant , k = ( 2.303 /t )x log ( M_o / M)

Where

M_o = initial concentration = 0.400 M

M = concentration after time t = ?

t = time = 175 min

k = rate constant = 0.0313 min^-1

Plug the values we get log ( M_o / M) = (kt) / 2.303

= ( 0.0313 x175) / 2.303

= 2.38

M_o / M = 10^2.38

= 240.65

M = M_o / 240.65

= 0.400 / 240.65

= 1.66x10^-3 M

Therefore the concentration of [A] after 175 min is 1.66x10^-3 M

queen_honey_blossom answered 2 years ago

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