Second photo is for problem 3 Thank you 1. (5 points) Excess Ca(I03)2 (s) is pla

Question

Second photo is for problem 3 Thank you 1. (5 points) Excess Ca(I03)2 (s) is placed in pure water. At equilibrium, the solution contains 0.011 MIO3. (aq). What is K for the reaction. Ca(103)2(s) Ca2+(aq) +2103°aq) 2. (5 points) Hydrogen iodide decomposes according to the equation 2 HI (g) H2 (g) + 12 (e), for which Ke-0.0156 at 400° C. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400° c. Calculate the concentration of HIlat equilibrium. vessel at 400° C. Calculate the concentration of HI at equilibrium. Consider the following gas-phase equilibrium: 3. (5 points)

Explanation / Answer

Q1

Ca(IO3)2

[IO3-] = 0.011 M of IO3- in equilibrium

so..

Ksp = [Ca+2][IO3-]^2

assume for 1 mol of Ca+2 there are 2 mol of IO3-

so

[Ca+2] = 1/2*0.011 = 0.0055 M

so..

Ksp = 0.0055*(0.011 ^2) = 6.65*10^-7

Q2.

Kc = [H2][I2] / [HI]^2

[HI] = 0.55/2 = 0.275 M

in equilibrium

[HI] = 0.275 - 2x

[H2] = x

[I2] = x

so

Kc = [H2][I2] / [HI]^2

0.0156 = x*x/(0.275 - 2x)^2

sqrt(0.0156 ) = x /(0.275 - 2x)

0.12489 ( (0.275 - 2x)) = x

0.12489 *0.275 - 2*0.12489 x = x

0.03434 -0.24978x = x

1.24978x = 0.03434

x = 0.03434 /(1.24978) = 0.0274768

then

[HI] = 0.275 - 2x = 0.275 -2*0.0274768 = 0.2200464M

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