50 mL of water at 48.9EC were mixed with 50 mL of water at 23.8EC in a calorimeter also at 23.8EC. The final temperature was 33.1EC. Assuming that neither the density of water nor its specific heat capacity change with temperature, calculate the total heat capacity of the calorimeter. (density of water = 1.00 g mL-1, specific heat capacity = 4.18 J g-1 K-1)

Question

50 mL of water at 48.9EC were mixed with 50 mL of water at 23.8EC in a calorimeter also at 23.8EC.  The final temperature was 33.1EC.  Assuming that neither the density of water nor its specific heat capacity change with temperature, calculate the total heat capacity of the calorimeter. (density of water = 1.00 g mL-1, specific heat capacity = 4.18 J g-1 K-1)

DrBob222 · Answer

heat lost by water + heat gained by calorimeter = 0 [(mass H2O x specific heat H2O x (Tfinal-Tinitial)] + [(Ccal*(Tfinal-Tinitial)] = 0

Maria · Answer

The ionic compund sometimes called yellow uranium is used to produce colored glazes for ceramics. It is 7.252% sodium, 75.084% uranium, 17.664% oxygen?

a. What is the empirical formula for this compound?

b. This compound has a molecular mass of 1268.06 g/mol, what is the molecuslar compound for this formula?

DrBob222 · Answer

It is better to post your own question instead of riding piggy back on another post. I've already answered your question above.