(a) What is the mass of water used in this experiment? (b) Calculate the amount
ID: 547729 • Letter: #
Question
(a) What is the mass of water used in this experiment?
(b) Calculate the amount of energy (heat) absorbed by the water.
(c) Calculate the heat capacity of the metal.
A 48.50 g sample of a metal is heated to 100°C then placed into 100.0 mL of water (initially at 25.7 oC). The metal and water were allowed to reach thermal equilibrium, determined to be at 27.8 C Assuming no heat lost to the environment, calculate the specific heat of the metal. (a) What is the mass of water used in this experiment? (b) Calculate the amount of energy (heat) absorbed by the water (c) Calculate the heat capacity of the metal.Explanation / Answer
(a)
water 1 mL = 1g
mass of water = 100 g
(b)
heat gained by water = heat lost my metal
So
heat gained by water = M C delta T
= 100 g * 4.18 J/g oC* ( 27.8 -25.7)
= 878 J
(c)
Will be equal to heat lost by metal
878 J = mC delta T
Put values
878 J = 48.50 g * C * (100-27.8)
C = 0.25 J/g oC
or 0.25 kJ/kg oC Answer
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