Question

A drop of water with a mass of 0.48 g is vaporized at 100 ∘C and condenses on the surface of a 55- g block of aluminum that is initially at 25 ∘C . If the heat released during condensation goes only toward heating the metal, what is the final temperature in Celsius of the metal block? (The specific heat capacity of aluminum is 0.903 J/(g⋅∘C ).)
Express the temperature in Celsius to two significant figures.

Answer 1

The final temperature in Celsius of the metal block is 49°C.

How to find the number of moles ?

Moles water = $\frac{\text{Given mass}}{\text{Molar Mass}}$

                     = $\frac{0.48\ g}{18\ \text{g/mol}}$

                     = 0.0266 moles  

                   

Heat lost by water = 0.0266 mol x 44.0 kJ/mol

                                = 1.17 kJ

                                = 1170 J           [1 kJ = 1000 J]

Heat lost = Heat gained

Heat gained by aluminum = 1170 J  

1170 = 55 x 0.903 (T - 25) = 49.7 T - 1242  

1170 + 1242 = 49.7 T  

T = 48.5°C (49°C at two significant figures)

Thus from the above conclusion we can say that The final temperature in Celsius of the metal block is 49°C.

Learn more about the Moles here: brainly.com/question/15356425

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