A key step in the extraction of iron metal from iron ore is: FeO_(s) + CO_(g) Fe

Question

A key step in the extraction of iron metal from iron ore is: FeO_(s) + CO_(g) Fe_(s) + CO_2 (g) K_p = 0.403 at 1000 degree C What are the equilibrium partial pressures of CO_(g) and CO_2(g) when 1.00 atm of CO_(g) is reacted with an excess of FeO_(s) at 1000 degree C? Hydrogen sulfide (H_2S) decomposes according to the following reaction with a K_c = 9.30 times 10^-8 at 700 degree C. If 0.450 mols of H_2S were placed in a 3.00 L container, what would the equilibrium pressure of H_2(g) be at 700 degree C?As part of your answer, clearly demonstrate if the "x-is-small" assumption is valid. 2 H_2 S_(g) 2 H_2 (g) + S_2 (g)

Explanation / Answer

Quesiton 1.

Kp = 0.403

Find P of each sample when

initially

P-CO = 1 atm

P-CO2 = 0 atm

in equilbirium

P-CO = 1 -x

P-CO2 = 0 + x

substitute in p

Kp = P-CO2 / P-CO

0.403 = (x)/(1-x)

0.403 -0.403 x = x

1.403 x = 0.403

x = 0.403 /1.403

x = 0.2872416

P-CO = 1 -x = 1-0.2872416 = 0.71275 atm

P-CO2 = 0 + x = 0.2872416 atm

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