Question

Assume that you are in charge of designing a process to produce acetylene (C₂H₂) from ethane (C₂H₆), which is the reverse of the reaction shown above. Use your knowledge of equiLiBrium to suggest a set of conditions that would maximize the concentration of acetylene (C₂H₂) at equiLiBrium. Assume that it is possible to add or remove any of the three components of this system and to change the general conditions of the reaction (pressure, temperature, volume). C₂H₂(g) + 2H₂(g) ⇌ C₂H₆(g) ΔH = ?

Answer 1

Maximizing acetylene from ethane requires increasing temperature, decreasing pressure, and removing hydrogen gas from the system to shift the reaction equilibrium in favor of acetylene formation according to Le Châtelier's principle.

Step-by-step explanation:

To maximize the concentration of acetylene (C₂H₂) from ethane (C₂H₆), we need to shift the equilibrium position of the reaction :

C₂H₂(g) + 2H₂(g) ⇌ C₂H₆(g) ΔH = -312.0 kJ/mol C₂H₂

Since the conversion of acetylene to ethane is exothermic (releases heat), according to Le Châtelier's principle, to drive the reaction in the reverse direction (to produce acetylene), we should apply conditions favoring endothermic processes. This suggests:

• Increase the temperature, which favors the endothermic reverse reaction.
• Reduce the pressure, which shifts equilibrium towards the side with fewer moles of gas (Acetylene and hydrogen combined have 3 moles vs. 1 mole of ethane).
• Remove H₂ as it is produced, thereby shifting equilibrium to the left to produce more acetylene.

However, this theoretical conversation might not be practical or feasible, as the direct reaction from carbon and hydrogen to form acetylene is complicated and not typically performed in a laboratory setting due to its low selectivity and yield.