Use the References to access important values if needed for this question. Use t

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Use the References to access important values if needed for this question. Use the Referencer oaccess important valuesirneeded for this question. Consider the following system at equilibrium where AH J 10.4 k J, and K 55.6, at 698 K. When 0.39 moles of I,(g) are added to the equilibrium system at constant temperature: the value of K A. increases. B. decreases C. remains the same. the value of Q A. is greater than K B. is equal to K C. is less than K. the reaction must A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. the concentration of H, will: A. increase. B. decrease. C. remain the same. Submit Answer Retry Entire Group 7 more group attempts remaining

Explanation / Answer

Solution :-

Reaction is at equilibrium initially therefore the Kc and Qc are same

The equilibrium constant dosent change with change in the concentrations therefore Kc will remain same

When we add 0.39 moles of I2(g) this means we are increasing the concentration of the reactant therefore to attain the new equilibrium reaction will proceed into the forward direction therefore the Qc of the reaction will increase. This means after adding the 0.39 mol I2(g) Qc will be less than Kc

Since reaction trying to attain new equilibrium by proceeding into forward direction that means

Reaction will run in the forward direction to reestablish equilibrium

When reaction proceed into forward direction then concentration of the H2 will decrease because it get used up in the reaction to form more products.

So here are the correct answer choices for the each part

The value of Kc = remains the same

The value of Qc = is less than Kc

The reaction must = run in the forward direction to reestablish equilibrium

The concentration of H2   = decrease

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