monium nitrate (NH.NO) is an ionic compound (i.e., a "salt) often used in cold paks. When NH.NO, solved in water, it dissociates into its constituent ions, followed by a temperature drop: NH.NO3 → NH4+ + NO3 you dissolve 32.0 g of ammonium nitrate (NH.NO) in a styrofoam coffee-cup calorimeter containing 175 g of water, and measure a temperature decreases of the water from 22.5 °C to 8.2 °C. Assume the specific heat of the final solution (i.e., the "system") is equal to that of water. Note that total mass (m) of the system = mass of water + mass of NH.NO. ✓ Recall the heat formula: 4 = (m) x (c) (T2-T1), where m = mass (grams); C = specific heat (water = 4.184/9°C); AT (°C) = T2 - TI. Answer the questions below and show all your work. 1. (a) Determine the beat change that occurred in the calorimeter. (D) is the "q" value a negative, or positive, number? 2. Is this an endothermic or exothermic reaction? Does heat flow from the surroundings to the system, or from the system to the surroundings? Explain in detail, justify your answer.