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For the equilibrium reactions A2(g) + B2(g) ⇌ 3C(g) ⇌ 2D(g), both steps are exothermic, so lower temperatures are favorable. In the first step, the number of moles increases, favoring lower pressure, while in the second step, the number of moles decreases, favoring higher pressure. What conditions are most suitable for these reactions?

1. Low temperature and high pressure
2. High temperature and low pressure
3. Low temperature and low pressure
4. High temperature and high pressure

Correct answer: Low temperature and high pressure

Solution

Since both steps are exothermic, low temperature is favorable. For step 1, low pressure is favorable due to an increase in moles, while for step 2, high pressure is favorable due to a decrease in moles. Overall, low temperature and high pressure are optimal.

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