Answer:
0.57J/g°C is the specific heat capacity of the metal.
Explanation:
Heat lost by metal will be equal to heat gained by the water
[tex]-Q_1=Q_2[/tex]
Mass of metal= [tex]m_1=36 g[/tex]
Specific heat capacity of metal= [tex]c_1=?[/tex]
Initial temperature of the metal= [tex]T_1=86^oC[/tex]
Final temperature = [tex]T_2=T=36^oC[/tex]
[tex]Q_1=m_1c_1\times (T-T_1)[/tex]
Mass of water= [tex]m_2=41 g[/tex]
Specific heat capacity of water= [tex]c_2=4.18 J/g^oC [/tex]
Initial temperature of the water = [tex]T_3=30^oC[/tex]
Final temperature of water = [tex]T_2=36^oC[/tex]
[tex]Q_2=m_2c_2\times (T-T_3)[/tex]
[tex]-Q_1=Q_2[/tex]
[tex]-(m_1c_1\times (T-T_1))=m_2c_2\times (T-T_3)[/tex]
On substituting all values:
[tex]-(36 g\times c_1\times (36^oC-86^oC))=41 g\times 4.18 J/g^oC\times (36^oC-30^oC)[/tex]
we get, [tex]c_2 =0.57J/g^oC[/tex]
0.57J/g°C is the specific heat capacity of the metal.
