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Magnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A coffee-cup calorimeter at 25 oC contains 15.0 mL of water at 25 oC. A 2.00 g sample of is dissolved in the water and 1.51 kJ of heat are evolved. You may make the following assumptions about the solution: volume = 15.0 mL, density = 1.00 g mL-1, specific heat = 4.18 J g-1 oC-1.

(a) What is the balanced equation for the dissolution process?

(b) Is the process exothermic or endothermic?

(c) What is the heat change of water?

(d) What is the final temperature of the solution

(e) What are the initial and final temperatures in oF?

 

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2 Dec 2020

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Related questions

Magnesium sulfate is often used in first-aid hot packs, giving off heat when dissolved in water. A coffee-cup calorimeter at 25 contains 15.0 mL of water at 25 . A 2.00-g sample of is dissolved in the water and 1.51 kJ of heat are evolved. (You can make the following assumptions about the solution: volume = 15.0 mL, density = 1.00 g/ml, specific heat = 4.18 )

a.) What is the balanced equation for the solution process?

b.) Is the process exothermic?

c.) What is  

d.) What is the final temperature of the solution?

e.) What are the initial and final temperatures in ?

A sample of nickel is heated to 99.8 oC and placed in a coffee cup calorimeter containing 150.0 g of water at 23.5 oC. After the metal cools, the final temperature of the metal and water mixture is  25.0 oC. If the specific heat of the nickel is 0.444 J/g oC and the specific heat of water is 4.18 J/g oC, what mass of nickel was originally heated? Assume that no heat was lost in the surroundings.

student Jorge performs an experiment in which he adds 11.40 g KNO3 to 63.80 mL of deionized water in a coffee cup calorimeter. He calculates the enthalpy change of the solution for the process to be +1818.31 J. This value can be expressed as the molar enthalpy change of dissolution for KNO3, in kJ/mol. What is Jorge's molar enthalpy change of dissolution (kJ/mol)? Express your response to two digits after the decimal.

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student Sarah is measuring the heat of dissolution of KNO3 in water. She adds 2.81 g of solid KNO3 to 41.75 mL of deionized water in a coffee cup calorimeter (mass of the coffee cups + the stir bar = 20.32 g). The initial temperature of the water is 56.33 oC, and the temperature of the solution after the dissolution process is complete is 11.52 oC. Assuming the specific heat of the solution is the same as that of pure water (4.184 J/g-K), what is the heat of solution for the dissolution process in J (Joules)?

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