2.85 × 10^22. A diamond with a mass of 0.568 g contains
2.85 × 10^22 atoms C.
Diamond is a form of pure carbon.
a) Convert <em>grams of C to moles of C</em>
Moles of C = 0.568 g C × (1 mol C/12.01 g C) = 0.047 29 mol C
b) Convert <em>moles of C to atoms of C
</em>
Atoms of C = 0.047 29 mol C × (6.022 × 10^23 atoms C)/(1 mol C)
= 2.85 × 10^22 atoms C
Answer: The equilibrium constant is 
Explanation:
Initial concentration of 
= 0.095 M
The given balanced equilibrium reaction is,
Initial conc. 0.095 M 0 M
At eqm. conc. (0.095-x) M (2x) M
Given : 2x = 0.0055
x = 0.00275
The expression for equilibrium constant for this reaction will be,
![K_c=\frac{[l]^2}{[I_2]}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5Bl%5D%5E2%7D%7B%5BI_2%5D%7D)
Now put all the given values in this expression, we get :
Thus the equilibrium constant is
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