# Problem: Consider the reactionNi (s) + 4 CO (g) → Ni(CO)4 (g).At 30°C and PCO = 1 atm, Ni reacts with CO (g) to form Ni(CO) 4 (g). At 200°C, Ni(CO)4 (g) decomposes to Ni (s) and CO (g). This means1. the forward reaction is endothermic.2. adding an inert gas like argon favors the forward reaction.3. the activation energy for the forward reaction is greater than for the reverse reaction.4. a decrease in pressure favors the forward reaction.5. K at 30°C is greater than K at 200°C.

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Consider the reaction

Ni (s) + 4 CO (g) → Ni(CO)(g).

At 30°C and PCO = 1 atm, Ni reacts with CO (g) to form Ni(CO) (g). At 200°C, Ni(CO)(g) decomposes to Ni (s) and CO (g). This means

1. the forward reaction is endothermic.

2. adding an inert gas like argon favors the forward reaction.

3. the activation energy for the forward reaction is greater than for the reverse reaction.

4. a decrease in pressure favors the forward reaction.

5. K at 30°C is greater than K at 200°C.

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Based on our data, we think this problem is relevant for Professor Kozliak's class at University of North Dakota.