Answer:
a) 0.3660 J/g°C is the specific heat for the metal.
b) 37.7 Joules energy would it take to raise the temperature of 10.7 grams of silver by 15.2°C.
c)The specific heat of silver is 0.2347 J/g°C.
Explanation:
Energy required to raise the temperature,Q = 47.0 J
Mass of the unknown metal = m = 10.7 g
Change in temperature = ΔT = 25.0°C - 13.0°C = 12°C
Specific heat of metal = c
\(Q=mc\Delta T\)
\(47.0 J=10.7 g\times c\times 12^oC\)
\(c=\frac{47.0 J}{10.7 g\times 12^oC}=0.3660 J/g^oC\)
0.3660 J/g°C is the specific heat for the metal.
b) The molar heat capacity of silver = \(c_m=25.35 J/mol^oC\)
Molar mass of silver ,M= 108 g/mol
Specific heat of silver = c = \(\frac{c_m}{M}=-\frac{25.35 J/mol^oC}{108 g/mol}=0.2347 J/g ^oC\)
Given mass of silver = m = 10.7 g
Change in temperature = ΔT = 15°C
Energy required to raise the temperature of silver = Q
\(Q=mc\Delta T\)
\(Q= 10.7 g\times 0.2347 J/g ^oC\times 15^oC\)
Q = 37.7 Joules
37.7 Joules energy would it take to raise the temperature of 10.7 grams of silver by 15.2°C.
c) The specific heat of silver is calculated in (b) part above.
Specific heat of silver = c = \(\frac{c_m}{M}=-\frac{25.35 J/mol^oC}{108 g/mol}=0.2347 J/g ^oC\)
