5.00 g of potassium hydroxide (molar mass = 56.1 g/mol) dissolves in 100.0 g of water and the temperature of the solution increases by 1.60oC. Calculate  ΔH for the reaction in kJ/mol of KOH .The specific heat capacity of the solution is 4.18 J/goC   ( Hint: the mass of the solution is 105g)      (Hint #2: is this + or -?) Your answer should be in kJ/mol and have 3 sig figs

4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6

2 A student determines the heat of dissolution of solid cobalt(II) sulfate using a coffee-cup calorimeter of negligible heat capacity. When 1.34 g of CoSO4(s) is dissolved in 101.00 g of water, the temperature of the solution increases from 25.00 to 26.69 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.

The ΔH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kJ/(mol NaOH). What is the final temperature of the solution when a 10.1-g sample of NaOH dissolves in 250.0 g of water with and initial temperature of 23.0 oC in a coffee-cup calorimeter? Assume that the solution has the same specific heat as liquid water, i.e., 4.18 J/g-K.

THERMODYNAMICS: A 1.09 g sample of acetic acid (HC2H302) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 KJPC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 24.3°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)

In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.0 rnL of 1.00 M HCI are mixed. Both solutions were originally at 24.6 °C. After the reaction, the final temperature is 31.3 °C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87 J/g-°C, calculate the ΔHneut/mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.

Ice at 0.0 °C is placed in a Styrofoam cup containing 372. g of a soft drink at 15.4 °C. The specific heat of the drink is about the same as that of water. Some ice remains after the ice and soft drink reach an equilibrium temperature of 0.0 °C. Determine the mass of ice that has melted. Ignore the heat capacity of the cup. (Hint: It takes 334 J to melt 1 g of ice at 0.0 °C.) Be sure your answer has the correct number of significant digits. Note: Reference the Phase change properties of pure substances table for additional information. 1 6.D g x10 Ś

Solid calcium chloride dissolves in water according to the equation below.CaCl2 (s) ➝ Ca+2 (aq) + 2 Cl – (aq)      ΔHº = –81.3 kJ/mol8.00 grams of solid CaCl2 dissolves in 45.0 grams of water initially at a temperature of 20.00 ºC in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter.[You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g·ºC)]Tfinal = Answer ºC

In a constant‑pressure calorimeter, 60.0 mL of 0.320 M Ba(OH)2 was added to 60.0 mL of 0.640 M HCl.The reaction caused the temperature of the solution to rise from 24.50 ∘C to 28.86 ∘C. If the solution has the same density and specific heat as water (1.00 g/mLand 4.184J/g⋅°C, respectively), what is ΔH for this reaction (per mole H2O produced)? Assume that the total volume is the sum of the individual volumes. ΔH= _________ kJ/mol H2O

When a 6.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 3.74 kJ · K¯¹, the temperature decreases by 0.400 K. Calculate the molar heat of solution of KSCN. ΔΗsoln = kJ/mol