A calorimetric determination of specific heat and enthalpy of solution was performed.

How would each of the following procedural changes affect (higher than the correct value, lower than the correct value, or no change) the value of the specific heat of the metal determined in this experiment? Explain reasoning.

1.) The tube containing the metal was not left in the water bath long enough to reach the same temperature as the bath (100 C).

2.) Some of the water was spilled before the final weighing.

How would each of the following procedural changes affect (higher in magnitude [so if the value is negative, it will be more negative] than the correct value, smaller in magnitude than the correct value, or no change) the value of the enthalpy of solution determined in this experiment? Explain reasoning.

1.) The mixture of water and ionic solid was not stirred sufficiently so as to dissolve the solid completely.

2.) Not all of the solid in the beaker was poured into the calorimeter.

1.) The tube containing the metal was not left in the water bath long enough to reach the same temperature as the bath (100 C).

If the tube containing the metal is not left in the water bath for a sufficient amount of time to reach the same temperature as the bath, it would result in a lower value for the specific heat of the metal determined in this experiment. This is because to accurately determine the specific heat of a material, it is essential for the metal to reach thermal equilibrium with the water bath, which is set at a specific temperature. If the metal does not reach the desired temperature, the heat transfer between the metal and the water bath will not be complete, leading to an incomplete measurement of the specific heat. As a result, the calculated specific heat will be lower than its actual value.

2.) Some of the water was spilled before the final weighing.
If some of the water is spilled before the final weighing, it would result in a higher value for the specific heat of the metal determined in this experiment. This is because the specific heat is calculated based on the mass and temperature change of the water. When water is spilled, the mass of the water used in the experiment is reduced, leading to an overestimation of the specific heat. Since the specific heat is inversely proportional to the mass of the water, a decrease in mass would result in an increase in the calculated specific heat value.

Now let's move on to the effect of procedural changes on the enthalpy of solution:

1.) The mixture of water and ionic solid was not stirred sufficiently so as to dissolve the solid completely.
If the mixture of water and ionic solid is not stirred sufficiently to dissolve the solid completely, it would result in a smaller magnitude of the calculated enthalpy of solution. This is because the enthalpy of solution is calculated based on the heat released or absorbed when a substance dissolves in a solvent. In order for the substance to completely dissolve, it is necessary to ensure that the stirring is sufficient to facilitate the dissolution process. If the stirring is not sufficient, the dissolution process may be incomplete, leading to a smaller magnitude of the measured enthalpy of solution.

2.) Not all of the solid in the beaker was poured into the calorimeter.
If not all of the solid in the beaker is poured into the calorimeter, it would result in no change in the calculated enthalpy of solution. This is because the enthalpy of solution is determined based on the heat released or absorbed by the complete dissolution of a specific amount of substance. Therefore, the amount of solid poured into the calorimeter does not directly affect the enthalpy of solution, as long as the dissolution is complete.