A 225-g sample of a substance is heated to 340 C and then plunged into a 105-g a

Question

A 225-g sample of a substance is heated to 340 C and then plunged into a 105-g aluminum calorimeter cup containing 195 g of water and a 17-g glass thermometer at 12.5 C. The final temperature is 35.0C. The value of specific heat for aluminium is 900 J/kgC , for glass is 840 J/kgC , and for water is 4186 J/kgC . Part A What is the specific heat of the substance? (Assume no water boils away.) Express your answer using three significant figures.

I got 268 my first try and it was wrong. I really need help on this

Explanation / Answer

Q is heat or energy , C is specific heat

Energy required to raise or degrade the temperature is Q(x,y) = Mass*t*C

Here by Question: Q(lost,substance)= Q1(gained, water) + Q2(gained, glass) + Q3(gained,aluminum)

0.225*305*Csubstance= 0.195*22.5*(Cwater) + 0.017*22.5*(Cglass) + 0.105*22.5*(Caluminium)

= 0.195*22.5*4184 + 0.017*22.5*840 + 0.105*22.5*900

= 20804.85 J

Csubstance = 20804.85/(.225*305)

= 303.1672 J/kg-0C

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