Consider the following system at equilibrium where Kc = 0.159 and delta H° = -111 kJ/mol at...

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Chemistry

Consider the following system at equilibrium where Kc= 0.159 and delta H° = -111kJ/mol at 723 K.

N2(g) + 3H2(g) = 2NH3(g)

The production of NH3(g) is favoredby:

Indicate True (T) or False (F)for each of the following:

___TF 1. increasing thetemperature.
___TF 2. decreasing the pressure(by changing the volume).
___TF 3. increasing thevolume.
___TF 4. addingNH3.
___TF 5. removingH2.

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3.9 Ratings (661 Votes)
The reversible reaction is N2 3H2 2NH3 H111kj Temperature is 723K Equilibrium constant Kc is 0 159 The production of ammonia will increase by 1 Increasing temperature False Since it is a exothermic reaction    See Answer
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