Question

At low to moderate pressures, the equilibrium state of the water-gas shift reversible reaction CO + H2O + CO2 + H2 is approximately described by the relation: Усо, Ун, 4020 K(T) = 0.0247 exp YcoYH20 T(K) where T is the reactor temperature, Ke is the reaction equilibrium constant, and yi is mole fraction of species i in the reactor contents at equilibrium. The feed to a batch shift reactor contains 20.0 mole% CO, 10.0% CO2, 40% water, and the balance inert gas. The reactor is maintained at T = 1000°C. Assume a basis of 1 mol feed: () a (a) Draw and label a flowchart of this process. (b) Calculate the total moles of gas in the reactor at equilibrium and then the equilibrium mole fractions of each species in the product.

Answer 1

The water-gas shift reaction equilibrium can be described using an equation and the equilibrium constant depends on temperature. To calculate the equilibrium mole fractions of each species, we can use the initial mole fractions from the feed to the reactor and substitute them into the equation.

Step-by-step explanation:

The water-gas shift reaction is represented by the equation: CO(g) + H₂O(g) = CO₂(g) + H₂(g). The equilibrium constant, K, for this reaction depends on temperature and is given by the relation: Ke = 0.0247 exp((YcoYH20/4020)T(K)).

To answer part (b) of the question, we need to calculate the equilibrium mole fractions of each species in the product. Given that the feed to the reactor contains 20.0 mole% CO, 10.0% CO₂, 40% water, and the balance inert gas, we can use these values as the initial mole fractions. By substituting the values into the equation, we can determine the equilibrium mole fractions of each species.