1. When 5.0 g of KOH were dissolved in 74.0 g water in a calorimeter at 23.9oC, the temperature of the solution went up to 37.8oC.
Is the solution endothermic or exothermic? Why?
2. When 5.0 g of KOH were dissolved in 74.0 g water in a calorimeter at 23.9oC, the temperature of the solution went up to 37.8oC.
What is ÎH for the solution of one mole KOH in water with the unit of KJ/mole?
3. A student obtained an unknown metal sample that weighed 65.3 g and at a temperature of 99.8oC, he placed it in a calorimeter containing 43.7 g of water at 25.7oC. At equilibrium the temperature of the water and metal was 34.5oC.
Knowing the specific heat of the water to be 4.18 J/goC, what is the specific heat of the metal?
[ Hint: S.H.water x mwater x Ît water= S.H.metal x mmetal x Ît metal ]
4. Assuming that KOH exists as K+ and OH- ions in solution, what is the equation that occurs when KOH is dissolved in water?
1. When 5.0 g of KOH were dissolved in 74.0 g water in a calorimeter at 23.9oC, the temperature of the solution went up to 37.8oC.
Is the solution endothermic or exothermic? Why?
2. When 5.0 g of KOH were dissolved in 74.0 g water in a calorimeter at 23.9oC, the temperature of the solution went up to 37.8oC.
What is ÎH for the solution of one mole KOH in water with the unit of KJ/mole?
3. A student obtained an unknown metal sample that weighed 65.3 g and at a temperature of 99.8oC, he placed it in a calorimeter containing 43.7 g of water at 25.7oC. At equilibrium the temperature of the water and metal was 34.5oC.
Knowing the specific heat of the water to be 4.18 J/goC, what is the specific heat of the metal?
[ Hint: S.H.water x mwater x Ît water= S.H.metal x mmetal x Ît metal ]
4. Assuming that KOH exists as K+ and OH- ions in solution, what is the equation that occurs when KOH is dissolved in water?