A 3.00 L flask initially contained 0.200 mol CO_2, mol CO, and 0.800 mol O_2 at

Question

A 3.00 L flask initially contained 0.200 mol CO_2, mol CO, and 0.800 mol O_2 at 2000 K. Given that the equilibrium constant (Kx) for the reaction: is 0.738 at 2000 K. Which of the following statements is true? The value of "Q" is and the. a) 0.333, concentration of CO_2 will decrease as the system approaches equilibrium b) 1.67, concentration of CO_2 will increase as the system approaches equilibrium c) 0.600, concentration of CO will increase as the system approaches equilibrium d) 5.00, concentration of CO will decrease as the system approaches equilibrium e) 5.00, concentration of CO will increase as the system approaches equilibrium

Explanation / Answer

2CO2 ----------> 2CO + O2

[CO]     = 0.5/3 = 0.167M

[O2]       = 0.8/3 = 0.267M

[CO2]    = 0.2/3   = 0.067M

Qc = [CO]2[O2]/[CO2]2

         = (0.167)2 *0.267/(0.067)2

            = 1.67

Kc   = 0.738

Qc>Kc    The quilibrium shift to left side.

b. 1.67 concentration of Co2 will be increases as the system approaches equilibrium.

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