The specific heat of a metal is determined by heating the weighed metal, adding
ID: 809864 • Letter: T
Question
The specific heat of a metal is determined by heating the weighed metal, adding it to water in a calorimeter, and measuring the temperature change. The specific heat of water is 4.180 Joules per g per C. The data collected are as follows:
Grams of water in the calorimeter 45.14
Grams of metal 19.01
Initial temperature of metal 99.56
Initial temperature of water (C) 22.14
Maximum temperature of water after metal is added (C) 23.59
Calculate the following:
(1) Temperature fall of metal
(2) Temperature rise of water
(3) Joules gained by water (= joules lost by metal)
(4) Specific heat of metal
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The heat of solution is found by adding a salt to water in a calorimeter and measuring the temperature change.
The specific heat of water is 4.180 Joules per g per C. In the calculation of the heat of solution, ignore the contribution to specific heat and mass due to the salt. Assume that these contributions are negligible.
The data collected are as follows:
Grams of water in the calorimeter 49.58
Grams of salt 4.4301
Initial temperature of water 22.42
Final Temperature 18.92
Calculate the following:
(5) Change in water temperature (C)
(6) Change in Joules in water
(7) Heat of solution of salt
Explanation / Answer
Temperature fall of metal
It will be equal to the temperature rise in water = 23.59 - 22.14oC = 1.45oC
Temperature rise of water
It will same as the final temp - initial temp = 23.59 - 22.14oC = 1.45oC
Joules gained by water (= joules lost by metal)
we know, Q = m x Cp x delta T
delta T = 1.45oC
m = mass of water = 45.14g
Cp = 4.18J/g/oC
So Q = 45.14 x 4.18 x 1.45 = 273.59J
Specific heat of metal
use Q = m x Cp x delta T
delta T = 1.45oC
m= mass of metal = 19.01g
Q = 273.59 J
So , Cp = Q/(mx delta T) = 273.59/ ( 19.01 x 1.45oC) = 9.925J/g/oC
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