Question

If the specific heat of gold is 0.13 J/gC, what is the amount of energy (heat) required to raise 30.0g of gold from 15 degrees Celsius to 41 degrees Celsius?

Answer 1

Answer: The amount of energy required is 101 Joules

Explanation:

The quantity of heat required to raise the temperature of a substance by one degree Celsius is called the specific heat capacity.

$Q=m\times c\times \Delta T$

Q = Heat absorbed = ?

m= mass of gold = 30.0 g

c = specific heat capacity of gold = $0.13J/g^0C$

Initial temperature of the water = $T_i$ = 15°C

Final temperature of the water = $T_f$  = 41°C

Change in temperature ,$\Delta T=T_f-T_i=(41-15)^0C=26^0C$

Putting in the values, we get:

$Q=30.0g\times 0.13J/g^0C\times 26^0C$

$Q=101J$

The amount of energy required is 101 Joules