Question

calculate δg o for each reaction using δg o f values: (a) h2(g) i2(s) → 2hi(g) 2.6 kj (b) mno2(s) 2co(g) → mn(s) 2co2(g) kj (c) nh4cl(s) → nh3(g) hcl(g) 91.2 kj standard thermodynamic values at 298 k substance δg o f (kj/mol) co(g) −137.2 co2(g) −394.4 co2(aq) −386.2 hcl(g) −95.30 hcl(aq) −131.17 hi(g) 1.3 mno2(s) −466.1 nh3(g) −16 nh3(aq) 26.7 nh4cl(s) −203.0

Answer 1

(a)The change in Gibbs free energy for the reaction has been 2.6 kJ/mol.

(b) The change in Gibbs free energy for the reaction has been -49.3 kJ/mol.

(c) The change in Gibbs free energy for the reaction has been 91.38 kJ/mol.