Question

One piece of copper jewelry at 101°C has twice the mass of another piece, which is at 38.0°C. Both pieces are placed inside a calorimeter of negligible heat capacity. What is the final temperature inside the calorimeter (c of copper=0.387 j/g.k)?

Answer 1

Answer:

80.0°C will be the final temperature inside the calorimeter.

Explanation:

Heat lost by  the pace of jewelry  will be equal to heat gained by the another piece of the jewelry

$-Q_1=Q_2$

Mass of piece-1= $m_1=2m$

Specific heat capacity of copper= $c$  = 0.387 J/g.K

Initial temperature of the iron = $T_1=101^oC$

Final temperature = $T_2$=T

$Q_1=m_1c_1\times (T-T_1)$

Mass of piece-2= $m_2=m$

Specific heat capacity of copper = $c$  = 0.387 J/g.K

Initial temperature of the water = $T_3=38.0^oC$

Final temperature of water = $T_2$=T

$Q_2=m_2c_2\times (T-T_3)$

$-Q_1=Q_2$  (conservation of energy)

$-(m_1c_1\times (T-T_1))=m_2c_2\times (T-T_3)$

On substituting all values:

$-(2mc\times (T-101^oC))=mc\times (T-38.0^oC)$

$T= 80.0^oC$

80.0°C will be the final temperature inside the calorimeter.