10.2k views
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? 839.52 J, released 419.76 J, absorbed 839.52 J, absorbed 419.76 J, released?

1 Answer

3 votes

Answer:

419.76 J absorbed

Step-by-step explanation:

In thermodynamics, the specific heat of a substance is the amount of energy required to raise 1 gram of the substance by one degree Celsius. The formula involving specific heat is Q = mCΔT, where Q is the amount of heat gained (absorbed) or lost (released) by the substance, m is the mass of the substance, C is the specific heat, and ΔT is the change in temperature.

We are already provided all the information we need to solve for Q, so we can plug the appropriate values into the equation:

  • Q = mCΔT
  • Q = (95.4 g)(0.44 J/g*⁰C)(32⁰C - 22⁰C)
  • Q = (41.976 J/⁰C)(10⁰C)
  • Q = 419.76 J

The last step of the problem is determining whether energy is absorbed or released. We calculated Q to be a positive value, which means that energy is absorbed. We also know energy is absorbed because the temperature of the nickel increased, meaning that it gained thermal energy.

User Bhupesh
by
8.1k points