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5 votes
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?

User Divibisan
by
7.9k points

2 Answers

7 votes

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

Solution :

Formula used :


Q=m* c* \Delta T=m* c* (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* 0.44J/g^oC* (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.

User Aswin Rajendiran
by
8.4k points
4 votes
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.
User Mirushaki
by
8.9k points
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