C(s) + H2O(g) → H2(g) + CO2(g)
ΔG for the reaction above at 1300k is -43KJ. At this temperature, the reaction is?

Dickson3030

9 years ago

the reaction is feasible because negative Gibb's free energy indicate dat d enthalpy of product is greater Dan d enthalpy of reactant hence feasible or possible reaction

Phourlar

12 years ago

Its exothermic

vickyf

9 years ago

ooh dats true

Chi4sure

2 years ago

Butt the they said when the free ∆G is positive the reaction is endothermic so i believe when it is negative the reaction should be spontaneous and exothermic

giwish

9 years ago

not feasible shud b d ansa,,,carbon cannot displace hydrogen...its nt exothermic cos ∆H was nt given only the free energy was indicated....optionA

vickyf

9 years ago

it is exothermic naw... myschool God bless u .....du d correction