A 500 gm sample of water is reacted with an equimolar amount of CaO (both at an initial temp of 2 5 ∘ C ). What is the final temperature of the product? [Assume that the product absorbs all of the hea

Question

A 500 gm sample of water is reacted with an equimolar amount of CaO (both at an initial temp of $2 5^{\circ} C$ ). What is the final temperature of the product?

[Assume that the product absorbs all of the heat released in the reaction]

[Heat produced per mol of $Ca (OH)_{2}$ is 65.2 kJ and specific heat $Ca (OH)_{2}$ is $1.2 J / g^{\circ} C$ .]

TestHub · Accepted Answer

No. of moles of H 2 ​ O = No. of moles of CaO = No. of moles Ca ( OH ) 2 ​ produced = 500/18 CaO + H 2 ​ O ⟶ Ca ( OH ) 2 ​ Total heat released = 18 500 ​ × 65.2 × 1000 J Mass of Ca ( OH ) 2 ​ produced = 18 500 ​ × 74 gm ​ ∴ 18 500 ​ × 74 × 1.2 × ( T − 25 ) = 18 500 ​ × 65.2 × 1000 ​ ​ 88.8 ( T − 25 ) = 65200 T = 734.23 + 25 ⇒ 759.2 3 ∘ C

Chemistry - Thermochemistry Question with Solution | TestHub

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