Answer: The amount of heat required is 116.5 Joules
Explanation:
To calculate the amount of heat absorbed, we use the equation:
[tex]q=m\times C\times \Delta T[/tex]
where,
q = amount of heat absorbed = ?
m = mass of metal = 15.2 g
C = specific heat capacity of metal = [tex]0.397J/g^oC[/tex]
[tex]\Delta T[/tex] = change in temperature = [tex](T_2-T_1)=(40.3-21.0)^oC=19.3^oC[/tex]
Putting all the values in above equation, we get:
[tex]q=15.2g\times 0.397J/g^oC\times 19.3^oC\\\\q=116.5J[/tex]
Hence, the amount of heat required is 116.5 Joules
