A generic solid, X, has a molar mass of 80.4 g/mol. In a constant-pressure calorimeter, 16.0...

A generic solid, X, has a molar mass of 80.4 g/mol. In a constant-pressure calorimeter, 16.0 g of X is dissolved in 337 g of water at 23.00 °C.

The temperature of the resulting solution rises to 28.70 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there\'s negligible heat loss to the surroundings. How much heat was absorbed by the solution?

how much heat was absoped

waht is the enthrapy

Solutions

Expert Solution

total mass of mixture = 337+16 = 353 g

initial temperature = 23 c

final temperature = 28.7 c

DT = 28.7 -23 = 5.7

heat released in the process (q) = m*s*DT

= 353*4.184*5.7

= 8.42 joule

no of mole of solid = 16/80.4 = 0.2 mole

DHsol = q/n = 8.42/0.2 = 42.1 kj/mol

queen_honey_blossom answered 10 months ago

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