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.

Question

Chemistry

Missy

2 August, 01:21

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.

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Answers (1)

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Grady Greene · Answer 1

26.6 s.

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