The decomposition reaction of a to b has a rate constant of 0.00132 s-1: a → 2b if the initial concentration of a is 0.156 m, how long will it take for the concentration of a to decrease by 78.1%

-

92.4 s

Explanation: -

The decomposition reaction of a → b has a rate constant k = 0.00132 s⁻¹

From the rate constant we see that the reaction is of zero order.

The rate equation for a zero order reaction is

A₀ - A = kt

where A₀ = initial concentration.

T = time passed since start of reaction,

A is the amount present after t time passed.

A₀ = 0.156 M

A = A₀ - 78.1% of A₀

  = 0.156 - x 0.156

 = 0.156 - 0.122

 = 0.034 M

Plugging into the formula

A₀ - A = kt

0.156 - 0.034 = 0.00132 x t

t =

= 92.4 s

t =

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

yes

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