A student is asked to determine the energy change when a 2.00 g sample of NH,NO, is dissolved in water to make 100. g of solution. The temperature data are shown in the graph. 24 23 22 Time Which of the following is the magnitude of the energy change, q, for the dissolution? (Assume that the heat capacity of the solution is 4.18 J/g°C.) 13.4 J 418 J 669 J 9280 J Temperature ("C)

A chemist dissolved an 10.8-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 23.9°C. Based on this, how much heat energy was required to dissolve the sample of KOH? Assume the specific heat of the solution is 4.184 J/g - °C. %3D =Db Calculate the heat of solution for KOH in kJ/mol. kJ/mol heat of solution =

A 10.1 g sample of NaOH is dissolved in 250.0 g of water in a coffee-cup calorimeter. The temperature increases from 23.0 °C to °C. Specific heat of liquid water is 4.18 J/g-K and AH for the dissolution of sodium hydroxide in water is 44.4 kJ/mol. A) 33.3 B 40.2 С) 33.7 35.2 24.0

from the reaction (the system) to the surroundings. What is the sighH UI ule enuldipy tlangt ( reaction? 2. A student performs a reaction and determines the enthalpy change (AH) to be 31.4 kJ. Will the temperature of the surrounding solution increase or decrease as a result of this chemical process? 3. If you hold 3 grams of ice in your hand at room temperature, your hand

When 5.325 g KCL dissolves in 100.0ml of water the temperature decreases from 24.1 c to 21.2 c. Calculate the change in enthalpy per mole of KCL. Determine if the process is endothermic or exothermic.

A chemist dissolved an 14.2-g sample of KOH in 100.0 grams of water in a coffee cup calorimeter. When she did so, the water temperature increased by 30.5 ∘C. Based on this, how much heat energy was required to dissolve the sample of KOH? Assume the specific heat of the solution is 4.184 J/g⋅°C. ?=   kJ Calculate the heat of solution for KOH in kJ/mol.

A solution is made by mixing 232.0 mL of ethanol initially at 12.7 ∘C with 232.0 mL of water initially at 22.5 ∘C. What is the final temperature of the solution assuming that no heat is lost? The density of ethanol is 0.789 g/mL and the density of water is 1.00 g/mL. The specific heat of ethanol is 2.46 J/g·°C and the specific heat of water is 4.184 J/g·°C ?f=        ∘C

2.568 g of a Strontium chloride was dissolved in 150.0 mL of water.  The initial temperature of the 150.0 mL of water was 18.2 ºC. When the strontium chloride was added, the temperature of the mixture increased to 24.8 ºC.     1. Calculate how much heat was absorbed by the solution when the salt dissolved.

The specific heat of substance C is 0.93 J/(g K) and that of substance D is 1.8 J/(g K). You are given an unknown that could be pure substance C, pure substance D, or a homogeneous mixture of C and D. In the lab you determine that it requires 23.3 J of heat energy to raise the temperature of a 25.0 g sample of the unknown by 1.0 K. What conclusions can you make about the identity of your unknown, from this data?

The enthalpy of solution (∆H) of KOH is -57.6 kJ/mol. If 3.21 g KOH is dissolved in enough water to make a 150.0 mL solution, what is the change in temperature (°C) of the solution? (The specific heat capacity of the solution is 4.184 J/g･°C and the density of the solution is 1.02 g/mL).