Question

Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of : ()()() Suppose a ⁢ flask is charged under these conditions with of ammonia. How much is left later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to significant digits.

Answer 1

Answer:

26.6 s.

Step-by-step explanation:

For a zero order kinetics, the formula is:

[A] = [A₀] - kt

where,

[A] = amount pr concentration left

[A₀] = initial concentration or amount

k = rate constant

t = time

concentration = mole/volume

[A₀] = 0.5/2.0

= 0.25 M

[A] = 0.25/2.0

= 0.125 M

k = 0.0047 Ms⁻¹

t = ([A] - [A₀]/-k

= (0.125 - 0.25)/(-0.0047)

= 26.60 s.

the amount is reduced by half after 26.6 seconds