A 6.22-Kg piece of copper metal (s=0.385J/(g°C) is heated from 20.5°C to 324.3°C. Calculate the heat absorbed (in KJ) by the metal.
Answers 1
where in, q = heat energy
m = mass
c = specific heat capacity
∆T = change in temperature
= Tf - Ti
Given: m = 6220g Cu
c = 0.385J/g°C
Ti = 20.5°C
Tf = 324.3°C
Note: Ti = initial temperature
Tf = final temperature
Note: The unit of specific heat is in grams(g), and the mass given is in kilograms(kg), therefore the mass given must be converted first into grams(g).
kg → g
6.22kg Cu × 1000g/1kg = 6220g Cu
Unknown: q = ?
Formula: q = mc∆T
Solution:
q = mc∆T
= (6220g Cu)(0.385J/g°C)
(324.3°C - 20.5°C)
= (6220g Cu)(0.385J/g°C)(303.8°C)
= 727509.86J
Note: Units of other term are cancelled out, so the unit for heat energy will remain which is Joules(J).
Note: The problem asked for heat energy to be in kilojoules(kj)
J → kj
727509.86J × 1kj / 1000J = 727.51kj
Final Answer: q = 727.51kj
Tip: Cancelation of units is applicable only if the other same unit is on the denominator.
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