A generic solid, X, has a molar mass of 59.5 g/mol. In a constant‑pressure calorimeter, 45.3 g of X is dissolved in 309 g of water at 23.00 °C.   X(s)⟶X(aq)   The temperature of the resulting solution rises to 25.00. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? ?=   kJ What is the enthalpy of the reaction?   Δ?rxn=    kJ/mol

A quantity of 85.0 mL of 0.600 M HCl is mixed with 85.0 mL of 0.600 M KOH in a constant-pressure  calorimeter. The initial temperature of both solutions is  the same at 17.35°C, and the final temperature of the  mixed solution is 19.02°C. What is the heat capacity of  the calorimeter? Assume that the specific heat of the solutions is the same as that of water and the molar heat of neutralization is −56.2 kJ/mol.

the molar heat capacity of iron is 25.10 J mol –1 K–1 . A 25.0 g ball is heated until it is glowing red (to a temperature of 400.°C). It is dropped into a 50.0 mL container of water at 25.0°C. If the density of water is 0.997 g mL–1 , and the molar heat capacity of water is 4.186 J g–1 K–1 , what temperature (in K) will the ball and water equilibrate to? A) 338 B) 300 C) 317 D) 359 E) 342

When 60.0 mL of a 0.400 M solution of HNO3(aq) is combined with 60.0 mL of a 0.400 M solution of NaOH(aq) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 °C. The initial temperature of the solutions is 24.0 °C. Calculate qrxn in joules, assuming the specific heat capacity of the final solution is 3.90 J.g-¹.°C-¹, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/°C. (Hint: start with 9rxn+qsoln+qcal = 0.) The balanced chemical equation for this reaction is: HNO3(aq) + NaOH(aq) → H₂O(1) + NaNO3 (aq)

100.0 mL of 1.00 M HBr at 22.5 °C is combined with 100.0 mL of 1.00 M LiOH at 22.5 °C. The mixture reaches a temperature of 29.2 °C. Assume the density of the solutions is 1.00 g/mL and their specific heat capacity is the same as pure water. What is the molar heat of reaction?

When a 7.00 g sample of KSCN is dissolved in water in a calorimeter that has a total heat capacity of 5.28 kJ⋅K^-1, the temperature decreases by 0.330 K Calculate the molar heat of solution of KSCN.

Determine the change in enthalpy (H, in J) transferred when 8.0 g of sucrose (C12H22O11)are dissolved in 92.0 g of water in a coffee cup calorimeter. The temperature of the solution changesfrom 15.0 °C to 14.7 °C Assume the process takes place at constant pressure, the masses areadditive, and the specific heat of the solution is 4.18 J/g∙°C.

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 0.79 g of KOH(s) are dissolved in 104.10 g of water, the temperature of the solution increases from 24.69 to 26.63 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.58 J/°C. Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol. Assume the specific heat of the solution is equal to the specific heat of water. kJ/mol AH dissolution = BrookaCom Cengage Leaming Thermometer Cardboard or Styrofoam lid Nested Styrofoam cups Reaction occurs in solution.

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 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 13.10 mL of 3.00 M HCI, both initially at room temperature (22.00 °C), the temperature increased to 29.60 °C. The resultant salt solution had a mass of 28.10 g and a specific heat capacity of 3.74 J K- g-. What is the heat capacity of the calorimeter (in J/°C)?Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ mol-1