Answer the following question, using the table below: If equal masses Al and Fe
ID: 1057570 • Letter: A
Question
Answer the following question, using the table below: If equal masses Al and Fe heated to the same temperature and are each dropped into separate beakers containing equal volumes of room temperature water, which beaker of water and metal will have the higher final temperature? Explain your answer. When 10 kg of metal X was heated to 80.0 degree C and dropped into 400 grams of water at 25.0 degree C, the final temperature of the metal and water was 56.8 degree C. What is the specific heat and identity of metal X? (The specific heat for H_2O = 4.185 J/g degree C.)Explanation / Answer
(a) Specific heat is the amount of heat required per unit mass to raise the temperature by one degree Celsius.
Al has higher specific heat than Fe, therefore Al has more heat energy when heated.
When both the metals dropped into water, Al will pass more energy to water, therefore will have higher final temperature.
(b) The heat energy will transfer from metal X to water.
Therefore we can say Qlost (metal) = Qgain (water)
QX = Qwater
Cp.mX.(TX - TF) = Cp.mW.( TF - TW)
Given, final temperature, TF = 56.8 oC and Cp (water) = 4.184.
Substitute,
Cp.(10) (80.0 - 56.8) = (4.186) (0.4) (56.8 - 25)
Cp = 0.23
Hence, metal X is Cd (Cadmium)
(25.0) (85.0 - x)(0.45) = (75.0) (x - 20.0) (4.184)