Compound mn decomposes to form m and n in a reaction that is first-order with respect to mn and first order overall. the half-life for the reaction is 2.3 × 10^4 s. what is the rate constant of this reaction at 25°c? mn → m + n a) 3.0 × 10^3 s b) 1.6 × 10^(–4) s^(–1) c) 3.0 × 10^(–5) s^(–1) d) 3.3 × 10^(–4) s^(–1)

Explanation:

The reaction given follows this pattern:

1) Decomposition reaction:

2) First-order kinetic with respect to MN and first-order overall:

                               t = τ

 ∴ τ =  ln(2) / k ⇒ k = ln (2) / τ =  ln(2) / 2.3 × 10⁴ s / ln(2) = 3.0 × 10⁻⁵ s⁻¹

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.