Question

Fill The ICE table, calculate the concentration of each gas, write Kc expression..?

Answer 1

• `K_c = (["CO"(g)] * ["H"_2"O" (g)])/(["CO"_2(g)] * ["H"_2(g)]`
• `c("CO") = c("H"_2"O")~~ 1.356 color(white)(l) "mol"`
• `c("CO"_2) = c("H"_2)~~ 2.644 color(white)(l) "mol"`

Explanation:

The equilibrium constant is the ratio of the product of the concentration of products (`"CO"(g)` and `"H"_2"O"(g)`) to that of the reactants (`"CO"_2(g)` and `"H"_2(g)`).

`color(white)(ll)` `"CO"(g) + "H"_2"O"(g) rightleftharpoons "CO"_2(g) + "H"_2(g)`
I #color(white)(l) 2.00 color(white)(l(g) +) 2.00 color(white)(l_2(g) rightleftharpoons) 2.00 color(white)(g")" +)2.00#
C #-x color(white)(l(g) +) -x color(white)(l(g) rightleftharpoons ) +x color(white)(g")" +) +x#
E `2.00 - x color(white)(lll) 2.00 - x color(white)(rightleftharpoons) 2.00 + x color(white)(l) 2.00 + x`

`((2.00 + x)^2)/((2.00 - x)^2) = K_c = 3.80`

`x ~~ 0.644 color(white)(l) "M"`

To calculate equilibrium concentrations, substitute `x` into expressions in the last row of the ICE table:

• `c("CO") = 2 - x ~~ 1.356 color(white)(l) "M"`

• `c("H"_2"O") = 2 - x~~ 1.356 color(white)(l) "M"`

• `c("CO"_2) = 2 + x ~~ 2.644 color(white)(l) "M"`

• `c("H"_2) = 2 + x ~~ 2.644 color(white)(l) "M"`