Question

The specific heat of zinc is 0.39 j/g*��

c. how much energy needed to change the temperature of 34g of zinc from 22��c to 57��
c. is the energy absorbed or released?

Answer 1

I just did this and the correct answer was 464.1 J, absorbed

Answer 2

Answer : The amount of energy needed are, 464.1 J and the value is positive that means the energy is absorbed.

Solution :

Formula used :

`Q=m* c* \Delta T=m* c* (T_(final)-T_(initial))`

where,

Q = energy gained or absorbed = ?

m = mass of zinc = 34 g

c = specific heat of zinc =
`0.39J/g^oC`

`\Delta T=\text{Change in temperature}`

`T_(final)` = final temperature =
`57^oC`

`T_(initial)` = initial temperature =
`22^oC`

Now put all the given values in the above formula, we get the energy gained or absorbed.

`Q=34g* 0.39J/g^oC* (57-22)^oC`

`Q=464.1J`

Therefore, the amount of energy needed are, 464.1 J and the value is positive that means the energy is absorbed.