A) A sealed container initially contains only 1.0 M gas A and 1.0 M gas B. Upon

Question

A) A sealed container initially contains only 1.0 M gas A and 1.0 M gas B. Upon heating the following reaction takes place: A(g) + 2 B(g) ? C(g)+ 2 D(l). After the reaction comes to equilibrium, the concentration of gas C is 0.25 M. What is the equilibrium constant Kc for this reaction?

B). The decomposition of N2O4 into NO2 has Kp = 2. Some N2O4 is placed into an empty container, and the partial pressure of NO2 at equilibrium is measured to be 0.2 atm. What was the initial pressure in the container prior to decomposition?

C). For the following reaction, find the value of Q and predict the direction of change, given that a 1L flask initially contains 2 moles S8, 2 moles SF6, and 2 moles F2.               

1/8 S8 (s) + 3 F2 (g) ? SF6 (g)   Kc = 0.425

D)

A key step in the extraction of iron from its ore is

FeO(s) + CO(g) ? Fe(s) + CO2(g) Kp =0.403 at 1000°C.

What are the equilibrium partial pressures off carbon monoxide and carbon dioxide when 1.00 atm of carbon monoxide and excess iron(II) oxide react in a sealed container at 1000°C.

Explanation / Answer

Ans A

Balanced reaction with ICE TABLE

A(g) + 2 B(g) ? C(g)+ 2 D(l)

I 1 1

C -x - 2x +x +2x

E. (1-x) (1-2x) x 2x

At equilibrium

Concentration of C = x = 0.25 M

Concentration of D = 2x = 2*0.25 = 0.50 M

Concentration of A = 1-x = 1-0.25 = 0.75 M

Concentration of B = 1-2x = 1-0.5 = 0.50 M

Equilibrium constant expression of the reaction

Kc = [D]2[C] / [B]2 [A]

= (0.50*0.50)*(0.25)/(0.50*0.50)*(0.75)

= 0.333

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