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32g of anhydrous copper(ii)tetraoxosulphate(vi) dissolved in 1dm³ of…

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32g of anhydrous copper(ii)tetraoxosulphate(vi) dissolved in 1dm³ of water generated 13.0kj of heat. The heat of solution is?

A. 26.0kj/mol

B. 65.0kj/mol

C. 130.0kj/mol

D. 260.0kj/mol

QUICK ANSWER…

B

DETAILS…

Simple and straight forward calculation, all we have to do here is to convert the 32g to mole, and the perform the heat of solution like this:

Heat of solution = heat generated / number of moles of CuSO4 dissolved

Data given:

Heat generated = 13KJ

Mass of CuSO4 dissolved = 32g

Molar mass of CuSO4 = 64 + 32 + 4(16) = 160g

This implies:

1 mole of CuSO4 = 160g, therefore,

X mole of CuSO4 = 32g

Cross multiplying to find X, we have:

32(1) = 160X

X = 32/160 = 0.2mole

This means the number of dissolved CuSO4 in moles = 0.2

Finally, heat of solution will be = 13/0.2 = 65KJ/mol

Now for the right answer to the above question:

  1. Option A is incorrect.
  2. Option B is correct.
  3. C is incorrect.
  4. D is not the correct answer.
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KEY-POINTS…

You may please note these/this:

  • Heat of solution = heat evolved / quantity dissolved in moles.
  • We did not use the volume of water given as 1dm3 because it is not necessary even from observing the unit.
  • In other to get the number of moles of the dissolved CuSO4, we would have to convert the dissolved mass given into moles bearing in mind that molar mass of it = 160g.
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/ culled from 2020 JAMB-UTME chemistry past question 25 /

32g of anhydrous copper(ii)tetraoxosulphate(vi) dissolved in 1dm³ of... » QuizTablet
32g of anhydrous copper(ii)tetraoxosulphate(vi) dissolved in 1dm³ of... » QuizTablet

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