l>2 K (s) + 2 H2O (ℓ) → 2 KOH (aq) + H2 (g) - Stoichiometry - Enthalpy • Entropy • Gibbs Free Energy - Equilibrium Constant

You are watching: K(s)+h2o(l)→koh(aq)+h2(g)

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Enter a mass or volume in one of the boxes below. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. All gases are assumed to be at STP.
 KMass: g H2OMass: g KOHMass: g H2Mass: g orGas Volume: L Heat Released: kJ

<2ΔHf(KOH (aq)) + 1ΔHf(H2 (g))> - <2ΔHf(K (s)) + 2ΔHf(H2O (ℓ))><2(-482.39) + 1(0)> - <2(0) + 2(-285.83)> = -393.12 kJ-393.12 kJ(exothermic)

<2ΔSf(KOH (aq)) + 1ΔSf(H2 (g))> - <2ΔSf(K (s)) + 2ΔSf(H2O (ℓ))><2(91.75) + 1(130.59)> - <2(64.68) + 2(69.91)> = 44.91 J/K44.91 J/K(increase in entropy)

From ΔGf° values:<2ΔGf(KOH (aq)) + 1ΔGf(H2 (g))> - <2ΔGf(K (s)) + 2ΔGf(H2O (ℓ))><2(-440.58) + 1(0)> - <2(0) + 2(-237.18)> = -406.8 kJ-406.80 kJ(spontaneous)

From ΔG = ΔH - TΔS:-406.51 kJ(spontaneous)

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