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.