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_2 (g) + 2H_2O (g) Certain changes (specified in the first column in the following table) are then made to this mixture. Considering each change separately, state the effect (increase, decrease, no change) that the change has on the original equilibrium value of the quantity in the second column (or K, if that is specified). The temperature and volume are constant. a) Predict whether the equilibrium for the following reaction will shift toward products or reactants with a temperature increase. CH_4(g) + H_2O(g) CO(g) + 3H_2(g) DeltaHdegree = + 206kJ b) Predict whether the equilibrium for the following reaction will shift toward products or reactants with a temperature increase. CO (g) + H_2O (g) CO_2 (g) + H_2 (g) DeltaHdegree = -41kJ

Explanation / Answer

Change

Quantity

Effect

Partial pressure of CO2 is increased

Partial pressure of CH4

decreases

Partial pressure of CH4 is decreased

Partial pressure of CO2

increases

Concentration of CO2 is increased

K

No change

Concentration of H2O is decreased

Concentration of CO2

increases

a)

Since heat is absorbed, with the increase in the temperature the equilibrium will shift towards products to counteract the change.

b)

Since heat is evolved, with the increase in the temperature the equilibrium will shift towards reactants to counteract the change.

Change

Quantity

Effect

Partial pressure of CO2 is increased

Partial pressure of CH4

decreases

Partial pressure of CH4 is decreased

Partial pressure of CO2

increases

Concentration of CO2 is increased

K

No change

Concentration of H2O is decreased

Concentration of CO2

increases

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