Chemistry: 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.

0.45 meters because millimeters are very tiny...

for the reaction, nh3(g) + hcl(g) nh4cl(s) run at

genyjoannerubiera

01.01.2022

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 1:

For the given chemical reaction:

$NH_3(g)+HCl(g)\rightarrow NH_4Cl(s)$

We are given:

$\Delta G$ = Gibbs free energy = -91368 J

T = Temperature = 25^oC=[273+25]K=298K

$\Delta S$ = entropy of the reaction = -284 J/K

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

$\Delta G=\Delta H-T\Delta S$

Putting values in above equation, we get:

$-91368J=\Delta H-(298K)(-284J/K)\\\\\Delta H=-176000J$

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

For 2:

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

Sign convention for $\Delta G$

If $\Delta G$ value comes out to be positive, it is considered as non-spontaneous reaction.If Delta G

value comes out to be negative, it is considered as spontaneous reaction.

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

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