A generic solid, X, has a molar mass of 58.9 g/mol. In a constant-pressure calorimeter, 30.9 g of X is dissolved in 259 g of water at 23.00 °C. X(s) → X(aq) The temperature of the resulting solution rises to 26.10 °C. 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? 9 = kJ What is the enthalpy of the reaction? AHrxn = kJ/mol

A generic solid, X, has a molar mass of 82.3 g/mol. In a constant-pressure calorimeter, 46.1 g of X is dissolved in 337 g of water at 23.00 °C. X(s) X(aq) The temperature of the resulting solution rises to 29.50 °C. 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? q = kJ What is the enthalpy of the reaction? AHrxn kJ/mol =

A 1.75 g sample of zinc metal is reacted with 128 g of 1.10 M hydrochloric acid solution in a constant-pressure calorimeter. The resulting solution changes in temperature from 22.58 °C to 22.97 °C. The hydrochloric acid is in excess. Based on this information, and estimating the solution's heat capacity as 4.18 Jg1 °C, what is the amount of heat, in joules, transferred in this reaction?

When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?

Iron has a specific heat capacity of 0.444J/g-C. 50.0 g of iron at 35C is added to 50.0 g of water with a specific heat capacity of 4.184 J/g-C. When the temperature of the resulting mixture stops changing, the temperature is closer to that of the original water than to the iron. True or false?

metal X =51.0g; specific heat capacity =0.44 J/C If metal X is heated to 86C and put into a calorimeter containing water (she=4.18 J/g°C ) at 23C. The final temperature of the water becomes 31C.   What is the mass of water?

[11] A 10.00 g sample of a metal alloy was heated to 88.99 °C. It is then quickly dropped into 40.0 g of water in a calorimeter. The water temperature rises from 19.73 °C to 24.23 °C. Calculate the specific heat of the alloy. [Specific Heat of Water = 4.184 J/g °C and Heat Capacity of Calorimeter = 12.6 J/°C]

A 0.770-g piece of lithium metal is dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0 °C. The reaction is 2 Li(s) + 2 H₂O(1)→ 2 LiOH(aq) + H₂(g) AHrxn=-446 kJ/mol Assuming no heat is lost to the surroundings, and that the final mixture has a specific heat capacity of 4.18 J/g °C, calculate the final temperature in °C. The enthalpy of fusion for ice is 6.02 kJ/mol.

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 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