85 mL of water is placed into a solution calorimeter. (The calorimeter is a styr

Question

85 mL of water is placed into a solution calorimeter. (The calorimeter is a styrofoam cup inside another styrofoam cup with solution in the bottom of one cup with a thermometer poked through a styrofoam cover). The temperature of this water is 22.3 degrees Celsius. When 5.97g of sodium sulfate (Na2SO4) are dissolved in this water, the temperature drops to 17.4 degrees Celsius. Please answer the following questions and show your work please. 1.) What is the temperature change(deltaT contents) of the calorimeter's contents? Be sure to give the proper sign for this quanity. 2.) What is the mass of the calorimeter's contents (mass contents)? 3.) What amount of heat (q contents) does the calorimeter's contents lose? Be sure to give the proper sign for this quanity. 4.) What amount of heat (q process) does the process of dissolving sodium sulfate in water absorb? Be sure to give the proper sign for this quanity. 5.) Compute the enthalpy of solution (delta H solution) for sodium sulfate. Be sure to give the proper sign for this quanity. 6.) Is this process of dissolving sodium sulfate in water exothermic or endothermic?

Explanation / Answer

1). delta T= 22.3-17.4=4.9 degree c

2). mass of calorimeter content=85+5.97

= 94.97 gm

3).q=-85*4.9 cal is lost by calorimeter content

4).q=85*4.9

5).delta H=-q

6).it is endothermic

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