What I have so far: Kc= [HI]^2/[H2][I2] Concentration (M) H2 + I2 <> 2HI 3.35. 3

Question

What I have so far: Kc= [HI]^2/[H2][I2] Concentration (M) H2 + I2 <> 2HI 3.35. 3.00 0
lD 99791965 Correct Hint 2. Determine the change in the concentration of iodine What value should be placed in the table in place of the "? for the change in concentration of the reactant 1? 2H1 Concentration (M) Initin Change Equilibrium H, 3.35 1, 3.00 + 0.0800 Be sure to include the sign of the change Express your answer with the appropriste units 2.92 M correct Use this value to determine the change in the concentration of hydrogen Hint 3. Determine the change in the concentration of hydrogen What value should be placed in tho table in place of the "7 for the change in concentration of the reactant H,? 2HI Coacentration (M) H Initial Change Equilibrium 3.00 2.92 0.0800 3.35 Be sure to include the sign of the change Express your answer with the appropriate units. , o ? |-3.24-1M Submit

Explanation / Answer

H2 (g)   + I2 (g)   <--------------->   2 HI (g)

3.35         3.00                                  0

-x             -x                                     +2x

3.35 - x     3.00 - x                           2x

At equilibrium :

[I2] = 3.00 - x = 0.08 M

x = 2.92

[H2] = 3.35 - 2.92 = 0.43 M

[HI] = 2 x 2.92 = 5.84 M

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

    = (5.84)^2 / (0.43 x 0.08)

Kc = 991

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