Question

The specific heat of nickel is 0.44 J/g*⁰C. How much energy needed to change the temperature of 95.4g of nickel from 22⁰C to 32⁰C. Is the energy absorbed or released?

Answer 1

To determine the heat or energy needed for the process, we use the equation,
                                               H  = mcpdT
where m is the mass, cp is the specific heat and dT is the temperature difference. 
                                               H = (95.4g)(0.44 J/g°C)(32°C - 22°C)
                                                   = 419.76 J
Thus, the amount of heat that should be ABSORBED is approximately 419.76 J. 

Answer 2

Answer : The amount of energy needed is, 419.76 J and the energy is absorbed.

Solution :

Formula used :

$Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})$

where,

Q = heat gained or absorbed = ?

m = mass of nickel = 95.4 g

c = specific heat of nickel = $0.44J/g^oC$      

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

$T_{final}$ = final temperature = $32^oC$

$T_{initial}$ = initial temperature = $22^oC$

Now put all the given values in the above formula, we get

$Q=95.4g\times 0.44J/g^oC\times (32-22)^oC$

$Q=419.76J$

The value of Q is positive that means energy is absorbed.

Therefore, the amount of energy needed is, 419.76 J and the energy is absorbed.