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a) A 430 mL  sample of water was cooled from 100.0 oC  to 30.0 oC . How much...

a) A 430 mL  sample of water was cooled from 100.0 oC  to 30.0 oC . How much heat was lost?

b) How many kilojoules are required to change the temperature of 26.5 g  of water from 19.8 oC  to 29.0 oC ?

c) Calculate the final temperature when 10 mL  of water at 80 oC  are added to 20 mL  of water at 25 oC

d) A piece of metal weighing 2.00 g  at a temperature of 41.0 oC  was placed in a calorimeter in 19.10 mL  of water at 18.9 oC . The final equilibrium temperature was found to be 26.7 oC . What is the specific heat of the metal?

e) If the specific heat of methanol is 2.51 J/K-g, how many joules are necessary to raise the temperature of 87 g  of methanol from 4 oC  to 99 oC ?

f) When a 3.78 g  sample of solid sodium hydroxide was dissolved in a calorimeter in 150.0 g  of water, the temperature rose from 14.5 oC  to 45.2 oC . Calculate ΔH (in kJ/mol NaOH) for the following solution process:

NaOH(s)→Na+(aq)+OH−(aq)

Assume that it’s a perfect calorimeter and that the specific heat of the solution is the same as that of pure water.

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as per HomeworkLib policy I have did 4 parts

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