Question

The equilibrium reaction below has the Kc = 4.00 at 25°C. If the temperature of the system at equilibrium is increased to 100°C, how and for what reason will the equilibrium shift. Also show and explain how and why the Kc value will change.

Answer 1

Following are the answer to this question:

Step-by-step explanation:

In the given question information is missing, that is equation which can be defined as follows:

`CH_4(g)+H_2O(g)\rightarrow CO(g)+3H_2(g) \ \ \bigtraingleup H^0=+206.2KJ`

• Growing temperatures may change its connection to just the way which consumes thermal energy in accordance with Le chatelier concepts Potential connection is endothermic. Answer: shifts to the right

• Kc are described as a related to the concentration by the intensity of both the reaction for each phrase which reaches a power equal towards its stoichiometric equation coefficient Kc = \frac{product}{reactant} It increases [product] but reduces [reactant] Therefore, Kc increases