An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calori

Question

An aluminum calorimeter with a mass of 100 g contains 250 g of water. The calorimeter and water are in thermal equilibrium at 10.0°C·Two metallic blocks are placed into the water. One is a 300.0-g piece of copper at 30.0°C. The other has a mass of 70.0 g and is originally at a temperature of 100°C The entire system stabilizes at a final temperature of 20.0°C. Specific Heats of Some Substances at 25°C and Atmospheric Pressure Specific Heat Specific Heat J/kg C C) Substance Elemental solids Aluminum Beryllium Cadmium Cop Germaniun Gold Iron Lead Silicon Silver 900 1 830 230 387 322 129 448 128 703 234 Substance Other solids Brass Glass Ice (-5) Marble Wood 380 837 2 090 860 1 700 er Liquids Alcohol (ethyl) Mercury Water (15 C) 2 400 140 4 186 Gas Steam (100 C) 2 010 Not: To convert values to units of cal/g·°C, divide by 4 195. (a) Determine the specific heat of the unknown sample J/kg °c

Explanation / Answer

Energy absorbed by aluminium and water

Q = (250 x 4.186 x (20 - 10)) + (100 x 0.900 x (20 - 10))

Q = 11365 J

Energy released by copper and unknown material.

Q = (300 x 0.387 x (30 - 20)) + (70 x C x (100 - 20))

Q = 1161 + 5600C

Assuming no heat loss

11365 = 1161 + 5600C

C = 1.82 J/kg deg C

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