## BaCl2 (aq) + 1 K2CrO4 (aq) → BaCrO4 (s) + 2 KCl (aq)

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## Reaction Type:

Double Displacement

## Stoichiometry

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 BaCl2          Mass: g or Solution Volume: mL of Concentration: mol/L K2CrO4         Mass: g or Solution Volume: mL of Concentration: mol/L BaCrO4         Mass: g KCl            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(BaCrO4 (s)) + 2ΔHf(KCl (aq))] - [1ΔHf(BaCl2 (aq)) + 1ΔHf(K2CrO4 (aq))]
[1(-1445.99) + 2(-419.55)] - [1(-871.9) + 1(-1385.95)] = -27.2399999999998 kJ
-27.24 kJ     (exothermic)

## Entropy Change

[1ΔSf(BaCrO4 (s)) + 2ΔSf(KCl (aq))] - [1ΔSf(BaCl2 (aq)) + 1ΔSf(K2CrO4 (aq))]
[1(158.57) + 2(158.98)] - [1(122.56) + 1(255.21)] = 98.76 J/K
98.76 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(BaCrO4 (s)) + 2ΔGf(KCl (aq))] - [1ΔGf(BaCl2 (aq)) + 1ΔGf(K2CrO4 (aq))]
[1(-1345.28) + 2(-414.55)] - [1(-823.3) + 1(-1294.45)] = -56.6300000000001 kJ
-56.63 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-56.69 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

8350237119.1
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 97.