C2H4(g)<----> C2H6 (g) + heat
what stresses would force the reaction to shift -> (to the right)?
a) pressure (increase/decrease):
b) temperature:
c) concentrations (of C2H6, C2H4, H2)
a) Pressure (increase): Increasing the pressure would push the reaction to shift to the right, according to Le Chatelier's Principle. By increasing the pressure, it would favor the side with fewer moles of gas to reduce the pressure.
b) Temperature: Increasing the temperature would push the reaction to shift to the right. This is an exothermic reaction, meaning it releases heat. According to Le Chatelier's Principle, increasing the temperature would favor the endothermic direction to absorb the excess heat.
c) Concentrations (of C2H6, C2H4, H2): Increasing the concentration of C2H6 or decreasing the concentration of C2H4 or H2 would push the reaction to shift to the right. According to Le Chatelier's Principle, increasing the concentration of a reactant or decreasing the concentration of a product would favor the forward reaction to consume the excess reactant or produce more product.