Acetic acid, which is used to make many important compounds, is produced from me
ID: 505484 • Letter: A
Question
Acetic acid, which is used to make many important compounds, is produced from methanol and carbon monoxide (which are themselves both derived from methane in natural gas) by a process called the Monsanto process. The endothermic reaction is run over a rhodium and iodine catalyst at 175 °C and 1 atm of pressure. Predict whether each of the following changes in the equilibrium system will shift the system to more products, to more reactants, or neither. Then explain each answer in two ways, (1) by applying Le Chatelier’s principle and (2) by describing the effect of the change on the forward and reverse reaction rates. CH3OH(g) + CO(g) + 207.9 kJ CH3CO2H(g) Rh/I2 175 °C 1 atm CH3OH(g) + CO(g) + 207.9 kJ Rh/I2 /=/ 175 °C CH3CO2H(g) a. The concentration of CO is increased by the addition of more CO. b. The concentration of CH3OH is decreased. c. The concentration of CH3CO2H(g) is decreased by removing the acetic acid as it forms. d. The temperature is decreased from 300 °C to 175 °C. e. The Rh/I2 catalyst is added to the equilibrium system. e. The Rh/I2 catalyst is added to the equilibrium system.
Explanation / Answer
For the given reaction -
a) The increasing of concentration of CO for the reaction shifts the equilibrium towards right (to form products)
b) The decreasing concentration of CH3OH shifts the equilibrium towards the formation of reactnats.
c) The decreasing concentration of acetic acid shifts the reaction towards the formation of products.
d) As the reaction is an endothermic reaction the decreasing concentration shifts the reaction towards to formation of reactants.
e) The catalyst fasten the reaction but there is no change the amount of reactnats/products.