The specific heat of nickel is 0.44 J/g°C. How much energy needed to change the temperature of 95.4g of nickel from 32°C to 22°C. Is the energy absorbed or released?

Question

Luna Chen · Accepted Answer

#419.76# #J#, Released.

We will first determine whether the energy is released or absorbed. The simplest method to determine that is to track the temperature shift. We can see that, #"Final Temperature " lt " Initial Temperature"#. Thus, the release of heat energy. Let's compute the heat now. We know, #"Heat Released or Absorbed by the Body " = "Mass of the Body" xx "Specific Heat of the Material" xx "Change in Temperature"#. Mathematically, #Q = msDeltaT# Now, Based on the Inquiry, #color(white)(xxx)Q = 95.4 * 0.44 * (22 - 32)# [As, #DeltaT = T_"final" - T_"initial"#] #rArr Q = -(95.4 * 0.44 * 10)# #rArr Q = -419.76# So, The Heat Energy Released is #419.76# #J#. The energy is released, as indicated by the negative sign. I hope this is useful.

Cooper Anderson · Answer

undefined To calculate the energy needed, use the formula: Q = mcΔT, where Q is the energy, m is the mass, c is the specific heat, and ΔT is the change in temperature.

Substitute the given values: m = 95.4g, c = 0.44 J/g°C, ΔT = (22°C - 32°C) = -10°C.

Q = (95.4g)(0.44 J/g°C)(-10°C) = -419.28 J.

The energy is absorbed because the temperature decreases, so the sign of the energy value is negative.