A 6.00 gram sample of solid gold was heated from 274 K to 325 K. How much energy was involved? Cs of gold is 0.129 J/g oC.

39.5J

Explanation:

Given parameters:

Mass of solid gold = 6g

Initial temperature = 274K

Final temperature = 325K

Specific heat capacity of gold = 0.129J/g°C

Unknown:

Amount of energy used = ?

Solution:

The amount of energy absorbed in changing in giving a temperature rise to a body is given as a product of its mass, specific heat capacity and change in temperature.

Mathematically;

H = m x C x Ф

where m is the mass of the body

c is the specific heat capacity

Ф is the change in temperature

Now the unknown is H;

We need to convert the given temperatures into °C from kelvin so we can work with it;

Initial temperature = 274K, in °C; 274 - 273 = 1°C

Final temperature = 325K, in °C; 325 - 273 = 52°C

Now input the parameters and solve;

H = 6 x 0.129 x (52 - 1) = 39.5J