for the reaction, nh3(g) + hcl(g) nh4cl(s) run at 25°c, δg = −91368 j and δs = −284 j/k. what is the enthalpy change for this reaction?
184,632 j
−91,084 j
−98,468 j
−176,000 j
true or false. a negative change in free energy, or −δg, represents a spontaneous reaction.

For 1: The enthalpy change for the given reaction is -176000 J.

For 2: Yes, the negative sign of the gibbs free energy represents a spontaneous reaction.

Explanation:

For the given chemical reaction:

We are given:

= Gibbs free energy = -91368 J

T = Temperature =

= entropy of the reaction = -284 J/K

To calculate the enthalpy of the reaction, we use the equation for gibbs free energy, which is:

Putting values in above equation, we get:

Hence, the enthalpy change for the given reaction is -176000 J.

Gibbs free energy is defined as the energy which is available to do some work. It is represented as

Sign convention for

So, yes the negative sign of the gibbs free energy represents a spontaneous reaction.

answer : a model is often used to explain and make things easier to understand when any scientific topic needs to be demonstrated and explained.

as in this case where a scientist wants to use a model to present the results of his detailed scientific investigation. he should do it as it will him to make the audience understand the concept in a much better way. also, it can be changed according to new scientific understandings.