13.7.2 Consider the following system at equilibrium where delta H degree = -87.9

Question

13.7.2

Consider the following system at equilibrium where delta H degree = -87.9 kJ/mol, and K_c = 1.20 times 10^-2, at 500 K. PCI_5(g) PCI_3(g) + CI_2(g) When 0.35 moles of PCI_5(g) are added to the equilibrium system at constant temperature: the value of K_c increases. decreases. remains the same. the value of Q_c is greater than K_c. is equal to K_c. is less than K_c. the reaction must: run in the forward direction to reestablish equilibrium. run in the reverse direction to reestablish equilibrium. remain the same, It is already at equilibrium. the concentration of NO will: increase. decrease. remain the same.

Explanation / Answer

effect of concentration doesn'the effect equilibrium constant of the reaction .here on addition of 0.35 moles of PCl5 the forward reaction rate increases to remove the concentration effect on reactant side

1) Value of Kc remains same

2) value of Qc also remains same

3) the reaction must run in forward direction to reestablish the equilibrium

4) PCl3 concentration will increases

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