Question

1. When a solid dissolves in water, heat may be evolved or absorbed. The heat of...

1.

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 6.20 g of CsClO4(s) are dissolved in 115.60 g of water, the temperature of the solution drops from 22.87 to 19.50 °C.

Based on the student's observation, calculate the enthalpy of dissolution of CsClO4(s) in kJ/mol.

Assume the specific heat of the solution is equal to the specific heat of water.

ΔHdissolution =  kJ/mol

2.

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 20.92 g of BaBr2(s) are dissolved in 111.60 g of water, the temperature of the solution increases from 22.47 to 25.54 °C.

Based on the student's observation, calculate the enthalpy of dissolution of BaBr2(s) in kJ/mol.

Assume the specific heat of the solution is equal to the specific heat of water.

ΔHdissolution =  kJ/mol

Homework Answers

Answer #2

answered by: anonymous
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution...
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 18.53 g of Cs2SO4(s) are dissolved in 100.40 g of water, the temperature of the solution drops from 25.54 to 22.92 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.85 J/°C....
When a solid dissolves in water, the solution may become hotter or colder. The dissolution enthalpy...
When a solid dissolves in water, the solution may become hotter or colder. The dissolution enthalpy (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 10.13 g K2SO4(s) is dissolved in 114.80 g water, the temperature of the solution drops from 24.11 to 20.86 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.77 J/°C. Based on...
A student determines the heat of dissolution of solid ammonium bromide using a coffee-cup calorimeter of...
A student determines the heat of dissolution of solid ammonium bromide using a coffee-cup calorimeter of negligible heat capacity. When 6.34 g of NH4Br(s) is dissolved in 119.00 g of water, the temperature of the solution drops from 25.00 to 22.76 °C. Based on the student's observation, calculate the enthalpy of dissolution of NH4Br(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. ΔHdissolution =  kJ/mol
The salt calcium bromide is soluble in water. When 1.48 g of CaBr2 is dissolved in...
The salt calcium bromide is soluble in water. When 1.48 g of CaBr2 is dissolved in 112.00 g of water, the temperature of the solution increases from 25.00 to 26.56 °C. Based on this observation, calculate the enthalpy of dissolution of CaBr2 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. ΔHdissolution =  kJ/mol
The salt cesium bromide is soluble in water. When 9.28 g of CsBr is dissolved in...
The salt cesium bromide is soluble in water. When 9.28 g of CsBr is dissolved in 115.00 g of water, the temperature of the solution decreases from 25.00 to 22.72 °C. Based on this observation, calculate the enthalpy of dissolution of CsBr (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. ΔHdissolution =  kJ/mol
When a 5.93-g sample of solid sodium hydroxide dissolves in 39.8 g of water in a...
When a 5.93-g sample of solid sodium hydroxide dissolves in 39.8 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 22.00 oC to 56.12 oC. Calculate H in kJ/mol NaOH for the solution process. NaOH(s) Na+(aq) + OH-(aq) The specific heat of water is 4.18 J/g-K.
When a 3.81-g sample of solid ammonium chloride dissolves in 57.9 g of water in a...
When a 3.81-g sample of solid ammonium chloride dissolves in 57.9 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 24.00 oC to 19.94 oC. Calculate H in kJ/mol NH4Cl for the solution process. NH4Cl(s) NH4+(aq) + Cl-(aq) The specific heat of water is 4.18 J/g-K.
When 7.56 g of NaCl is added to a coffee cup calorimeter, the water temperature changes...
When 7.56 g of NaCl is added to a coffee cup calorimeter, the water temperature changes by 4.1 ºC. If the heat of solution (the enthalpy change upon dissolving in water) is 3.8 kJ/mol, what mass of solution must be in the cup? Assume the specific heat capacity of the solution is the same as the specific heat capacity of water.
When a 4.00-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a...
When a 4.00-g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter (see figure below), the temperature drops from 23.0°C to 16.4°C. Calculate ΔH (in kJ/mol NH4NO3) for the solution process shown below. Assume that the specific heat of the solution is the same as that of pure water. Hint: this process occurs at constant pressure.
The enthalpy change for the dissolution of NH4NO3 is +26.8 kJ/mol. When 40.0 g of NH4NO3...
The enthalpy change for the dissolution of NH4NO3 is +26.8 kJ/mol. When 40.0 g of NH4NO3 dissolves in 250.0 g of water in a coffee cup calorimeter, what will the final temperature of a solution be if it was initially at 25.0 °C? Assume that the heat capacity of the solution is the same as the specific heat of pure water, 4.184 J/(g·K). Hint: don't forget to add the masses of solute and solvent.