Kevin+and+Brad


 * The Question**: When dissolving a solute that creates an endothermic reaction with the solvent, how does the molality affect the temperature of the solution?


 * In this experiment:**

The solution (endothermic reaction) used: Dissolving AMMONIUM CHLORIDE in WATER. ( NH4Cl(aq) > NH4+ (aq) + Cl- (aq) ) ( NH4 +(aq) + H2O > NH3 (aq) + H3O+ )

Dependent Variable: molality of ammonium chloride Independent Variables: to be determined after analyzing the temperature/time graphs produced from experiment.

Measuring devises: Vernier temperature probe, Electronic scale Containers: Beaker, Plastic plate and spoon, Mortar and pestle Chemicals: Distilled Water, Solid Ammonium Chloride
 * Materials:**


 * Procedure:**

(will be made by video, the word description is for now) 1.  Prepare 0.1 kg of water in a beaker. 2.  Put the temperature probe in the water. Make sure it’s all connected to the interface, with a computer ready to collect data. 3.  Prepare 26.725 (which would make a 5m solution put into 0.1kg of water) grams of ammonium chloride, and powder it. 4.  Start collecting temperatures for sixty seconds as you pour the ammonium chloride into the water.

- Rumgods, aka Chris, Yuup and Chaz think this is an interesting experiment and has done well with data collection but would like to see some analysis maybe?
 * Peer Comments**


 * Data we have so far:**