A 500 gm sample of water is reacted with an equimolar amount of `CaO` (both at an initial temp of `25^(@)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^(@)C`.

Options

A. `~~735^(@)C`
B. `~~760^(@)C`
C. `~~746^(@)C`
D. `~~789^(@)C`

Answer

B

Explanation

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,rarr,Ca(OH)_(2)):}`
Total heat released `=500/18 xx65.2xx1000 J`
Mass of `Ca(OH)_(2)` produced `=500/18xx74 gm`
`:." "500/18xx74xx1.2xx(T-25)=500/18xx65.2xx1000`
`88.8 (T-25)=65200" "," "T=734.23+25 rArr 759.23^(@)C`