Question

Coal can be used to generate hydrogen gas (a potential fuel) by thefollowing endothermic reaction.
C(s) + H2O (g) <==> CO(g) + H2(g)

if this reaction mixture is at equilibrium, predict whether each ofthe following will result in the formation of additional hydrogengas, the formation of less hydrogen gas, or have no effect on thequantity og hydrogen gas.

a. adding more C to the reaction mixture
b. adding more H2O to the reaction mixture
c. raising the temperature of the reaction mixture
d. increasing the volume of the reaction mixture
e. adding a catalyst to the reaction mixture
f. adding an inert gas to the reaction mixture

Answer 1

Answer:The statements b,c,d would lead to increased formation of more hydrogen gas and statements a, e and f would  lead to unchanged hydrogen concentration

Explanation:

Lechateliers principle can be used here to determine the effect  of changes observed in the system.

Lechateliers principle states that if  any reaction at equilibrium  is subjected to change in concentration, temperature and pressure or even in reaction conditions  then the equilibrium of the reaction would shift in such a way so that it can oppose the change .

So if any disturbance is caused to a reaction  at equilibrium hence  the equilibrium of reaction would shift in such a way so that it can counter balance the change caused to the reaction.

The above reaction is following:

C(s)+H₂O(g)→CO(g)+H₂(g)

The enthalpy change  of this reaction is positive and hence the reaction is endothermic in nature.

So the given changes would lead to the following  results:

a The addition of more amount of carbon C(s) would not lead to any further formation of hydrogen because carbon is added in solid state and Hydrogen gas is in gaseous state so the equilibrium for this given reaction would only change on addition of gaseous reactants as that would only lead to change in concentration.

b Since H₂O(g) is in gaseous state and a reactant and hence the addition of  H₂O(g) that is more reactant would lead to more formation of hydrogen gas according to lechatelier principle. The equilibrium would shift in such a way so that it can decrease the concentration of added H₂O(g) hence it would form H₂(g).

c Since the above reaction is endothermic in nature hence increasing the temperature of reaction would also shift the equilibrium of reaction towards more formation of H₂(g) that is in forward direction.

d When we increase the volume of reaction mixture that is we are increasing the amount of reactants hence the reaction would shift towards more formation of hydorgen gas.

e The catalyst does not change the position of equilibrium and hence no shift in position of equilibrium would be observed.So amount of hydrogen gas formed would remain unchanged.

f The addition of inert gas would not lead to any change to the reaction and equilibrium would be unaffected. Hence the formation of hydrogen gas would remain unchanged.

Answer 2

The study of chemicals and the bond is called chemistry. When the amount of the reactant and the product get equal is said to be equilibrium.

The correct answer is b, c, d would lead to increased formation of more hydrogen gas, and statements a, e and f would lead to unchanged hydrogen concentration.

According to the principle can be used here to determine the effect of changes observed in the system.

What is an endothermic reaction?

• Those reactions that require energy or temperature to complete the reaction are called endothermic reactions.
• The principle states that if any reaction at equilibrium is subjected to change in Concentration, Temperature, Pressure, or even in reaction conditions then the equilibrium of the reaction would shift in such a way so that it can oppose the change.

So if any disturbance is caused to a reaction at equilibrium hence the equilibrium of reaction would shift in such a way so that it can counterbalance the change caused to the reaction.

The reaction is as follows:-

$C(s)+H_2O(g)---->CO(g)+H_2(g)$

The enthalpy change of this reaction is positive and hence the reaction is endothermic in nature.

So the given changes would lead to the following results:

A. The addition of more amount of carbon C(s) would not lead to any further formation of hydrogen because carbon is added in solid-state. Hydrogen gas is in the gaseous state so the equilibrium for this given reaction would only change on the addition of gaseous reactants as that would only lead to a change in concentration.

B. Since H₂O(g) is in a gaseous state and a reactant and hence the addition of  H₂O(g) that is more reactant would lead to more formation of hydrogen gas according to the principle. The equilibrium would shift in such a way so that it can decrease the concentration of added H₂O(g) hence it would form H₂(g).

C . Since the above reaction is endothermic in nature hence increasing the temperature of the reaction would also shift the equilibrium of reaction towards more formation of H₂(g) that is in the forward direction.

D. When we increase the volume of the reaction mixture that is we are increasing the number of reactants hence the reaction would shift towards more formation of hydrogen gas.

E. The catalyst does not change the position of equilibrium and hence no shift in the position of equilibrium would be observed. So the amount of hydrogen gas formed would remain unchanged.

F. The addition of inert gas would not lead to any change to the reaction and equilibrium would be unaffected. Hence the formation of hydrogen gas would remain unchanged.

Hence, the correct answer is mentioned above.

For more information about the endothermic reaction, refer to the link:-https://brainly.com/question/2192784