Question

. Calculate ΔG for the following reaction at 25°C. Will the reaction occur (be spontaneous)? How do you know? NH3(g) + HCl(g) → NH4Cl(s) ΔH = -176.0 kJ ΔS = -284.8 J·K-1

Answer 1

Answer:

$\triangle G = -911.296 \ kJ$

Explanation:

ΔG = ΔH-TΔS

Where ΔH = -176 kJ = -176000 J , T = 25°C + 273 = 298 K , ΔS = -284.8 JK⁻¹

=> $\triangle G =-176000 - (298)(-284.8)$

=> $\triangle G = -176000+84870.4$

=> $\triangle G = -91129.6 \ J$

=> $\triangle G = -911.296\ kJ$

Since the value is negative, the reaction is spontaneous under standard conditions at 298 K and the reactants have more free energy than the products.