C2H4(g)<----> C2H6 (g) + heat
what stresses would force the reaction to shift -> (to the right)?
Several factors can force the reaction to shift to the right, increasing the production of C2H6 gas:
1) Decrease in ethane concentration: Le Chatelier's principle states that if a reactant is removed, the equilibrium will shift in the direction that produces more of that reactant. So, if ethane (C2H6) is removed from the system, the reaction will shift to the right to produce more C2H6 to replenish the removed reactant.
2) Increase in ethylene concentration: Similarly, if the concentration of ethylene (C2H4) is increased, the equilibrium will shift to the right to consume the additional C2H4 and produce more C2H6.
3) Decrease in pressure: According to Le Chatelier's principle, if the pressure is decreased, the equilibrium will shift in the direction that decreases the number of moles of gas. As the reaction to the right produces more moles of gas (one mole of C2H4 vs. two moles of C2H6), decreasing the pressure will favor the production of C2H6.
4) Increase in temperature: In this reaction, heat is released when C2H6 is formed. So, if the temperature is increased, the equilibrium will shift to the right to consume the excess heat and produce more C2H6.
It is important to note that these factors affect the position of equilibrium and do not affect the value of the equilibrium constant (K).