Consider the reaction of peroxydisulfate ion (s2o2−8) with iodide ion (i−) in aqueous solution: s2o2−8(aq)+3i−(aq)→2so2−4(aq)+i−3(a q). at a particular temperature the rate of disappearance of s2o2−8 varies with reactant concentrations in the following manner: experiment s2o2−8(m) i−(m) initial rate (m/s) 1 0.018 0.036 2.6×10−6 2 0.027 0.036 3.9×10−6 3 0.036 0.054 7.8×10−6 4 0.050 0.072 1.4×10−5 what is the rate of disappearance of i− when [s2o2−8]= 1.8×10−2 m and [i−]= 5.0×10−2 m ?

r = 3.61x M/s

Explanation:

The rate of disappearance (r) is given by the multiplication of the concentrations of the reagents, each one raised of the coefficient of the reaction.

r = k.

K is the constant of the reaction, and doesn't depends on the concentrations. First, let's find the coefficients x and y. Let's use the first and the second experiments, and lets divide 1º by 2º :

x = 1

Now, to find the coefficient y let's do the same for the experiments 1 and 3:

y = 1

Now, we need to calculate the constant k in whatever experiment. Using the first :

k = 4.01x10^{-3} M^{-1}s^{-1}[/tex]

Using the data given,

r =

r = 3.61x M/s

a. hope i'm right

explanation:

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.