Question

*For the process, NH₃ (g) + HCl (g) →NH₄Cl (s), which is right?*

1️⃣ ΔH > 0 ; ΔS > 0
2️⃣ ΔH < 0 ; ΔS > 0
3️⃣ ΔH > 0 ; ΔS < 0
4️⃣ ΔH < 0 ; ΔS < 0​

Answer 1

what is the question?

I didn't understand

Answer 2

Answer:

For the reaction NH

4

Cl(S)→NH

3

(g)+HCl(g) at 25

0

C, enthalpy change △=+177kJmol

−1

and entropy change △S=+285JK

−1

mol

−1

. Calculate free energy change △G at 25

0

C and product whether the reaction is spontaneous or not.Given, △H=177 kJ/mol, △S=285 JK

−1

mol

−1

, T=298 K

Using the relation, △G=△H−T△S

△G=(177×10

3

J/mol)−(298 K)(285 JK

−1

mol

−1

)

△G=92070 J/mole

△G=92.07 kJ/mole

△G>0

Since △G is positive, Hence reaction is non spontaneous.

mark me as brainlist

hope it helps you all thank you