Chemistry, asked by anterpreetkaur6, 4 months ago

reaction at equilibrium at 298 K has entropy change of 200 J. What will be the change in its enthalpy.​

Answers

Answered by miglanibhumi7
1

Answer:

Hey mate there is ur answer

Explanation:

In a spontaneous change, Gibbs energy always decreases and never increases. This of course reflects the fact that the entropy of the world behaves in the exact opposite way (owing to the negative sign in the TΔS term).

H2O(l)→H2O(s)(18.6.1)

water below its freezing point undergoes a decrease in its entropy, but the heat released into the surroundings more than compensates for this, so the entropy of the world increases, the free energy of the H2O diminishes, and the process proceeds spontaneously.

Note

In a spontaneous change, Gibbs energy always decreases and never increases.

An important consequence of the one-way downward path of the free energy is that once it reaches its minimum possible value, all net change comes to a halt. This, of course, represents the state of chemical equilibrium. These relations are nicely summarized as follows:

ΔG < 0: reaction can spontaneously proceed to the right:

A→B(18.6.2)

ΔG > 0: reaction can spontaneously proceed to the left:

A←B(18.6.3)

ΔG = 0: the reaction is at equilibrium; the quantities of [A] and [B] will not change

Recall the condition for spontaneous change

ΔG=ΔH–TΔS<0(18.6.4)

it is apparent that the temperature dependence of ΔG depends almost entirely on the entropy change associated with the process. (We say "almost" because the values of ΔH and ΔS are themselves slightly temperature dependent; both gradually increase with temperature). In particular, notice that in the above equation the sign of the entropy change determines whether the reaction becomes more or less spontaneous as the temperature is raised. For any given reaction, the sign of ΔH can also be positive or negative. This means that there are four possibilities for the influence that temperature can have on the spontaneity of a process.

The following cases generalizes these relations for the four sign-combinations of ΔH and ΔS. (Note that use of the standard ΔH° and ΔS° values in the example reactions is not strictly correct here, and can yield misleading results when used generally.)

> 0

Under these conditions, both the ΔH and TΔS terms will be negative, so ΔG will be negative regardless of the temperature. An exothermic reaction whose entropy increases will be spontaneous at all temperatures.

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