Consider mixture B, which will cause the net reaction to proceed forward. \\matr

Question

Consider mixture B, which will cause the net reaction to proceed forward. matrix{& & m net ightarrow & & cr { m Concentration}~(M) & m [XY] & ightleftharpoons & m [X] & + & m [Y] cr hfill m initial!: & 0.500 & & 0.100 & & 0.100 cr hfill m change!: & -x & & +x & & +x cr hfill m equilibrium!: & 0.500-x & & 0.100+x & & 0.100+x} The change in concentration, x, is negative for the reactants because they are consumed and positive for the products because they are produced. Part B Based on a K_c value of 0.180 and the given data table, what are the equilibrium concentrations of m XY, m X, and m Y, respectively? Express the molar concentrations numerically. m [XY], m [X], m [Y] =

Explanation / Answer

Kc = 0.18 = (0.1+X)^2 / (0.5-X) ......=> X = 0.151 M .......=> [XY] = 0.349 M .......[X] = 0.251 M = [Y]

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