Estimate the temperature where Delta G = 0 for the following reaction (Given: Delta H=-176 and Delta S = -284.5 J/K

NH3 + HCl --> NH4Cl

dG = dH - TdS

You know dG = 0, dH, and dS, solve for T (in kelvin).
I note you don't have any units for dH but I assume that is -176 kJ/mol. If that is so you will need to convert dS to kJ/mol before you do the calculation.

To estimate the temperature at which ΔG = 0 for the given reaction (NH3 + HCl → NH4Cl), we can use the equation:

ΔG = ΔH - TΔS

Where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, ΔS is the change in entropy, and T is the temperature in Kelvin.

We are given ΔH = -176 J and ΔS = -284.5 J/K.

When ΔG = 0, the equation becomes:

0 = -176 - T(-284.5)

To find the temperature (T), we can rearrange the equation:

0 = -176 + 284.5T

Rearranging further:

284.5T = 176

T = 176 / 284.5

Simplifying:

T ≈ 0.618 K

Therefore, the estimated temperature where ΔG = 0 for the reaction NH3 + HCl → NH4Cl is approximately 0.618 Kelvin.

To estimate the temperature where ΔG (Gibbs free energy) is equal to zero for the given reaction, we can use the equation:

ΔG = ΔH - TΔS

where:
ΔG = Gibbs free energy
ΔH = enthalpy change
T = temperature (in Kelvin)
ΔS = entropy change

Given:
ΔH = -176 J
ΔS = -284.5 J/K

When ΔG is zero, we have:

0 = ΔH - TΔS

Rearranging the equation, we get:

TΔS = ΔH

Now, we can solve for the temperature T:

T = ΔH / ΔS

Substituting the given values:

T = -176 J / -284.5 J/K

By canceling out the units, we can calculate:

T ≈ 0.62 K

Therefore, the estimated temperature where ΔG = 0 for the given reaction is approximately 0.62 Kelvin.