When a 12.5 g sample of NaOH(s) dissolves in 367.0 mL water in a coffee cup calorimeter, the temperature of the water changes from 21.6°C to 30.4°C. N2OH(s) → Na* (ag) + OH¯(ag) Assuming that the specific heat capacity of the solution is the same as for water (4.184 J/8.°C) and the density of the solution is 1.030 g/mL, calculate the following. a the heat transfer from system to surroundings (in J) b. AH for the reaction (in kJ) kJ

The reaction of zinc with hydrochloric acid is represented by the reactionZn(s) + 2 HCl(aq) ↔ ZnCl 2(aq) + H 2(g) -- ΔH = -152.5 kJ How many grams of zinc reacted with an excess of HCl (100.0 mL) if the temperature of the calorimeter increased from 25.0°C to 35.85 °C? Assume the heat capacity of the solution is the same as pure water (4.184 J/g*°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.

When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 3.95 g of CuCl2(s) are dissolved in 108.60 g of water, the temperature of the solution increases from 23.05 to 26.27 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.86 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of CuCl,(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. AHdissolution kJ/mol

Part A A silver block, initially at 55.8 °C, is submerged into 100.0 g of water at 24.1°C in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.3 °C. The specific heat capacities for water and silver are = 4.18 J/(g ·°C) and 0.235 J/(g·°C). What is the mass of the silver block? Express your answer to two significant figures and include the appropriate units. Cs, water • View Available Hint(s) Cs, silver = HA ? Value Units m =

Adding 4.88 g of NH4NO3 (s) to 140 g of water in a coffee-cup calorimeter (with stirring to dissolve the salt) resulted in a decrease in temperature from 19.0 °C to 16.7 °C. Calculate the enthalpy change for dissolving NH4NO3 (s) in water in kJ/mol. Assume the solution (whose mass is 144.9 g) has a specific heat capacity of 4.2 J/g. K. (Cold packs take advantage of the fact that dissolving ammonium nitrate in water is an endothermic process.) ACE A cold pack uses the endothermic enthalpy of a solution of ammonium nitrate. Enthalpy change = esc A kJ/mol @2 2 W S #3 E D 20 F3 $ 4 888 F4 R F do LO % 5 Cengage Learning Cengage Technical Support T G MacBook Pro 6 F6 Y v lo 7 H 38 F7 U CO DII F8 F9 K F10 L P F11 { Save and Exit F12

In a constant pressure coffee-cup calorimeter, 100.0 mL of 0. 050 M of Ag+ was mixed with 100.0 ml of 0.050 M of Cl‒. The temperature changed from 298.5 K to 299.4 K. Calculate the enthalpy of reaction, ΔH (kJ/mol). Assume that the solutions have a density of water (1 g/mL) and specific heat capacity of water (4.184 J/g °C).                                        Ag+(aq) + Cl‒(aq) ⟶ AgCl(s)