Instant cold packs used to treat athletic injuries contain solid nh4no3 and a pouch of water. when the pack is squeezed, the pouch breaks and the solid dissolves, lowering the temperature because of the endothermic reaction nh4no3(s)+h2o(l)→nh4no3(aq) δh= +25.7 kj.

what is the final temperature in a squeezed cold pack that contains 43.0 g of nh4no3 dissolved in 125 ml of water? assume a specific heat of 4.18j/(g⋅∘c) for the solution, an initial temperature of 27.5 ∘c, and no heat transfer between the cold pack and the environment.