The four gases CH_4, O_2, CO_2 and H_2O are mixed in a reaction vessel and allow

Question

The four gases CH_4, O_2, CO_2 and H_2O are mixed in a reaction vessel and allowed to reach equilibrium in the reaction CH_4(g) + 2O_2(g) = Co(g)+2H_2O(g) Certain changes (specified in the first column in the following table) are then made to The mixture. Considering each change separately, state the effectt (increase, decrease, no change) that the change has on the original equilibrium value o f the quantity in the second column (or K, if that is specified). The temperature and volume are constant. Predict whether the equilibrium for the following reaction will shift toward products or reactants with a temperature increase CH_4(g) + H_O(g) = CO(g) + 3H_2(g) DeltaH degree = +206 kJ Predict whether the equilibrium for the following reaction will shift toward products or reactants with a temperature. CO(g) + H_2O(g) = CO_2(g) + H_2(g) Delta H degree = +41kJ

Explanation / Answer

(4)

* Increase in partial pressure of CO2 Shifts the equilibrium towards left side hence increase the partial pressure of CH4

* Decrease in partial pressure of H2O Shifts the equilibrium towards right side hence increase the partial pressure of CO2

(a) Since the farward is endothermic reaction hence increase in temperature shifts the reaction towards endothermic i.e products side.

(b) Since the farward is exothermic reaction hence increase in temperature shifts the reaction towards endothermic i.e reactants side.

* As long as temerature is kept constant the equilibrium constant value is constant. Hence no effect.

* Increase in partial pressure of CH4 Shifts the equilibrium towards left side hence increase the partial pressure of CO2

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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