For the answer to the question above,
in this problem we can use the concept of freezing point depression since we are given the freezing point of the solution.
ΔT = -k(f) x m x i
-2.24 - 0 = -1.86 x m x 3
<span>m = 0.4014
</span>So the answer to your question is m = 0.4014
Answer:
they have same atomic number as they are the same element & electrons
Molar mass AgNO3 = <span>169.87 g/mol
1 mole AgNO3 ------------ 169.87 g
?? moles AgNO3 --------- 25.4 g
25.4 x 1 / 169.89 => 0.1495 moles</span>
Answer: The equilibrium constant is ![3.3\times 10^{-4}](https://tex.z-dn.net/?f=3.3%5Ctimes%2010%5E%7B-4%7D)
Explanation:
Initial concentration of
= 0.095 M
The given balanced equilibrium reaction is,
![I_2(g)\rightleftharpoons 2I(g)](https://tex.z-dn.net/?f=I_2%28g%29%5Crightleftharpoons%202I%28g%29)
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,
Now put all the given values in this expression, we get :
![K_c=\frac{(0.0055)^2}{(0.095-0.00275)}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%280.0055%29%5E2%7D%7B%280.095-0.00275%29%7D)
![K_c=\frac{(0.0055)^2}{0.09225}=0.00033](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%280.0055%29%5E2%7D%7B0.09225%7D%3D0.00033)
Thus the equilibrium constant is ![3.3\times 10^{-4}](https://tex.z-dn.net/?f=3.3%5Ctimes%2010%5E%7B-4%7D)