The decomposition of hydrogen iodide on a gold surface at 150 °c hi(g)½ h2(g) + ½ i2(g) is zero order in hi with a rate constant of 1.20×10-4 m s-1. if the initial concentration of hi is 0.373 m, the concentration of hi will be 0.0053 m after 2.64×103 seconds have passed. based on these data, the rate constant for the reaction is s-1.

k = 1,39x10⁻⁴Ms⁻¹

Explanation:

For the reaction:

HI(g) → ½ H2(g) + ½ I2(g)

The zero order formula is:

[A] = [A]₀ - kt

Where [A] is the concentration in time, t, [A]₀ is initial concentration and k is rate constant.

When [A]₀=0,373M, At t=2,64x10³ s, [A] is 0,0053M

Replacing:

0,0053M = 0,373M - k×2,64x10³s

0,3677M = k×2,64x10³s

k = 1,39x10⁻⁴Ms⁻¹

I hope it helps!

the increase of protons   hope this

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-