A 1.9 kgkg block of iron at 29 ∘C∘C is rapidly heated by a torch such that 17 kJkJ is transferred to it. What temperature would the block of iron reach (assuming the complete transfer of heat and no loss to the surroundings)? If that same amount of heat (17 kJkJ ) was quickly transferred to a 890 gg pellet of copper at 29 ∘C∘C, what temperature would the copper reach before it begins losing heat to the surroundings? Use the equation for heat capacity and the following heat capacity values: qcs, Fe(s)cs, Cu(s)===mcsΔT0.450 J/(g⋅∘C)0.385 J/(g⋅∘C) Express the final temperatures of the iron and copper in ∘C∘C to two significant figures separated by a comma. View Available Hint(s) Final temperatures of FeFe, CuCu = ∘C∘C
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
A 1.9 kgkg block of iron at 29 ∘C∘C is rapidly heated by a torch such that 17 kJkJ is transferred to it. What temperature would the block of iron reach (assuming the complete transfer of heat and no loss to the surroundings)? If that same amount of heat (17 kJkJ ) was quickly transferred to a 890 gg pellet of copper at 29 ∘C∘C, what temperature would the copper reach before it begins losing heat to the surroundings? Use the equation for heat capacity and the following heat capacity values:
qcs, Fe(s)cs, Cu(s)===mcsΔT0.450 J/(g⋅∘C)0.385 J/(g⋅∘C)
|
||||
|
Final temperatures of FeFe, CuCu =
|
|
∘C∘C
|
Trending now
This is a popular solution!
Step by step
Solved in 4 steps
