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Consider the dissolution of 1.50 grams of salt XY in 75.0 mL of water within a calorimeter. The temperature of the water decreased by 0.93 oC. The heat capacity of the calorimeter is 42.2 J/oC. The density of the water (and the solution) is 1.00 g/mL. The specific heat capacity of the solution is 4.184 J/goC. Calculate the quantity of heat lost by the surroundings.

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jufsanabriasa

Answer:

The quantity of heat lost by the surroundings is 258,5J

Explanation:

The dissolution of salt XY is endothermic because the water temperature decreased.

The total heat consumed by the dissolution process is:

4,184 J/g°C × (75,0 + 1,50 g) × 0,93°C = 297,7 J

This heat is consumed by the calorimeter and by the surroundings.

The heat consumed by the calorimeter is:

42,2 J/°C × (0,93°C) = 39,2 J

That means that the quantity of heat lost by the surroundings is:

297,7J - 39,2J = 258,5 J

I hope it helps!

Eduard22sly

The quantity of heat lost by the surroundings is 258.424 J

How to determine the mass of the water

  • Density of water = 1 g/mL
  • Volume of water = 75 mL
  • Mass of water =?

Mass = Density × Volume

Mass of water = 1 × 75

Mass of water = 75 g

How to determine the total heat consumed

  • Mass of water = 75 g
  • Mass of salt =  1.50 g
  • Mass of solution = 75 + 1.5 = 76.5 g
  • Temperature change (ΔT) = 0.93 °C
  • Specific heat capacity of the solution = 4.184 J/gºC
  • Total Heat (Q) =?

Q = MCΔT

Q = 76.5 × 4.184 × 0.93

Q = 297.67 J

How to determine the heat consumed by the calorimeter

  • Heat capacity of the calorimeter (C) = 42.2 J/ºC
  • Temperature change (ΔT) = 0.93 °C
  • Heat by calorimeter (H) =?

H = CΔT

H = 42.2 × 0.93

H = 39.246 J

How to determine the heat lost by the surrounding

  • Total Heat (Q) = 297.67 J
  • Heat by calorimeter (H) = 39.246 J
  • Heat lost by surrounding =?

Heat lost by surrounding = 297.67 – 39.246

Heat lost by surrounding = 258.424 J

Learn more about heat transfer:

https://brainly.com/question/6363778

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