Chemistry
Chemistry, 17.10.2019 22:40, Barton9720

If some of the salt remains adhered to the weighing paper (and therefore is not transferred to the calorimeter), will the enthalpy of solution for the salt be reported too high or too low?

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Chemistry, 18.10.2019 21:20, Tristabergeron5650
In a coffee-cup calorimeter, 1.62 g is mixed with 74.1 g water at an initial temperature of 25.44°c. after dissolution of the salt, the final temperature of the calorimeter contents is 23.33°c. assuming the solution has a heat capacity of 4.18 j/°c·g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of in units of kj/mol.
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Chemistry, 19.10.2019 03:10, s73588
This question has multiple parts. a. in a coffee-cup calorimeter, 1.81 g nh4no3 was mixed with 85.00 g water at an initial temperature 25.00oc. after dissolution of the salt, the final temperature of the calorimeter contents was 23.34oc. assuming the solution has a heat capacity of 4.18 j/g∙oc, and assuming no heat loss to the calorimeter, calculate the enthalpy of solution (∆hsoln) for the dissolution of nh4no3 in units of kj/mol. ∆ = kj/mol b. in a coffee-cup calorimeter, 1.81 g nh4no3 was mixed with 85.00 g water at an initial temperature 25.00oc. after dissolution of the salt, the final temperature of the calorimeter contents was 23.34oc. if the enthalpy of hydration for nh4no3 is -630. kj/mol, calculate the lattice energy of nh4no3. lattice energy = kj/mol
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Chemistry, 29.10.2019 07:31, acavalieri72
Consider the dissolution of 2.50 grams of salt xy in 75.0 ml of water within a calorimeter. the temperature of the water decreased by 0.93 oc. the heat capacity of the calorimeter is 42.2 j/oc. the density of the water (and the solution) is 1.00 g/ml. the specific heat capacity of the solution is 4.184 j/goc. calculate the enthalpy change for dissolving this salt on a energy per mass basis (units of j/g).
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