50. The following reaction is important in the synthetic fuels industry. This re

Question

50. The following reaction is important in the synthetic fuels industry. This reaction is also being looked at as the first step in converting carbon dioxide in the atmosphere in gasoline and other fuels, from which it come. The carbon monoxide obtained by running the reaction backwards may be reacted to give hydrocarbons. Here is the reaction: CO(g)+ H0(g)CO2(g) + H2(g) a. Consider the case in which the reaction is at equilibrium. Then each of the following changes are made. Explain how the partial pressure of each of the other chemicals are affected (increase, decrease or stay the same) as the system tries to move back to equilibrium. i. The partial pressure of water vapor is lowered ii. The partial pressure of carbon dioxide is lowered iii. More hydrogen is added to the reaction mixture iv. Hydrogen is removed from the reaction mixture b. The objective is to make carbon monoxide from carbon dioxide. In order to do this, how should the partial pressures of each chemical compare with that of carbon monoxide (higher, lower, much lower, much higher?)

Explanation / Answer

a) At equilibrium,

equilibrium constant=Kp=p(CO2)*p(H2)/p(CO)*p(H2O)

Le Chatlier's principle: The equilibrium shifts in the suitable direction ,which helps counteract the change in concentration/pressure of reactants/products

i) p(H2O) lowered (H2O is the reactant),the equilibrium will shift in the reverse direction.

reactants ,pCO and p(H2O) will increase while product pCO2 and pH2 will decrease as the equilibrium is re-established.(Le Chatlier's principle)

ii) p(CO2) lowered (CO2 is the product) ,the equilibrium will shift in the forward direction.

reactants ,pCO and p(H2O) will decrease while product pCO2 and pH2 will increase as the equilibrium is re-established.(Le Chatlier's principle)

iii)pH2 (product ) is increased,the equilibrium will shift in the reverse direction.

reactants ,pCO and p(H2O) will increase while product pCO2 and pH2 will decrease as the equilibrium is re-established.(Le Chatlier's principle)

iv) pH2 (product ) is removed,the equilibrium will shift in forward direction and go to completion

reactants ,pCO and p(H2O) will decrease while product pCO2 and pH2 will increase as the equilibrium is re-established.(Le Chatlier's principle)

b)partial pressure of products must he higher than that of reaction ,so that the equilibrium shifts in the forward direction

pCO and p(H2O) must be lower than pCO2 and pH2

Related Questions

Navigate

• Browse (All)
• Browse 5
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.