balanced chemical equation for dehydration: k3[Fe(C2O4)3].3H2O --> K3[Fe(C2O4)3]

Question

balanced chemical equation for dehydration: k3[Fe(C2O4)3].3H2O --> K3[Fe(C2O4)3] + 3H2O results: weight of container 38.185g,,, ,weight of container and hydrated salt: 39.700g,,,,, weight of hydrated salt: 1.515g,,,, moles of hydrated salt: 0.00308 mol,,,, weight of container and anhydrous salt: 39.559,,,, weight of anhydrous salt:1.374 weight of H2O lost: 0.141,,, what is moles of anhydrous salt? what is moles of H2O lost?? what is moles of water released per mole anhydrous salt?? what is the theoretical weight percent of hydrated salt? show caculations!!!!

Explanation / Answer

k3[Fe(C2O4)3].3H2O --> K3[Fe(C2O4)3] + 3H2O weight o f hydrated salt = 39.7 - 38.185 = 1.515 gms moles of anhydrous salt = weight of anhydrous salt/molar mass = 1.374/437.24 = 0.00314 moles of H2O lost = 0.141/18 = 0.007833 moles of water released per mole anhydrous salt = 0.0078/0.0031 = 2.4947

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