Chemistry
posted by Phillip .
A 32.5g cube of aluminum initially at 45.8 C is submerged into 105.3g water at 15.4 C. What is the final temp of both substances at thermal equilibrium. Assume the al and the H2O are thermally isolated from everything else)
Specific heat cap Al= .903
Specific heat cap H2O= 4.18
I understand this problem but In my math i get to:
(DeltaT) Al = 14.998 X (DeltaT) H2O
And im lost. Anyone able to explain the completion of the problem? Any help is greatly appreciated

You need to use TfinalTinitial for delta T.
heat lost by Al + heat gained by water=0
[mass Al x specific heat Al x (TfinalTinitial)] + [mass H2O x specific heat H2O x (TfinalTinitial)] = 0
Substitute and solve for Tf. 
I'm having trouble once i get to
T(final)=14.998 X T(final) + 14.998 X T(initial h2o) + T(initial Al)
Any suggestions? 
Yes. I think it is tough to try to manipulate the algebra. It is much easier to substitute the numbers first and manipulate them.
[32.5 x 0.903 x (Tf45.8)]+[105.3 x 4.18 x (Tf15.4)] = 0
29.35Tf  1344.1 + 440.15Tf  6778.4 = 0
Check those numbers to make sure I didn't make an error on my calculator, then solve for Tf. 
Thank you so much DrBob!
I ended up with
469.5Tf = 8122.54
Tf = 17.3
Thanks again,
Phil
Respond to this Question
Similar Questions

chem
A 25.0 g aluminum block is warmed to 65.2 C and plunged into an insulated beaker containing 55.3g of water initially at 22.0C. the aluminum and water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is … 
physic
Hi! Help me please, thank you so much. What mass of water at 28.0 °C must be allowed to come to thermal equilibrium with a 2.05kg cube of aluminum initially at 1.50 102 °C to lower the temperature of the aluminum to 54.8 °C? 
physic
What mass of water at 22.0 °C must be allowed to come to thermal equilibrium with a 1.66kg cube of aluminum initially at 1.50 multiplied by 102 °C to lower the temperature of the aluminum to 57.1 °C? 
Chemistry
a 15.7 g aluminum block is warmed to 53.2 degrees celsius and plunged into an insulated beaker containing 32.5 g of water initially at 24.5 degrees celsius. the aluminum and the water are allowed to come to thermal equilibrium. assuming … 
Physics
a): Two 50 g ice cubes are dropped into 200 g of water in a thermally insulated container. If the water is initially at 25 degree Celsius, and the ice comes directly from a freezer at 15 degree Celsius, what is the final temperature … 
Chemistry
Will someone show me the formula or help me through working this question? 
Chemistry
When 4.62 mL of cold water at 22.6 °C is mixed with 37.5 mL of hot water at 67.9 °C in a thermally isolated calorimeter, what is the final temperature of the mixture when thermal equilibrium has been achieved? 
Chemistry
A hot lump of 25.6 g of aluminum at an initial temperature of 57.4 °C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water given that the … 
Chemistry
A hot lump of 25.6 g of aluminum at an initial temperature of 57.4 °C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water given that the … 
Chemistry
A 32.3 g iron rod, initially at 22.4 ∘C, is submerged into an unknown mass of water at 62.9 ∘C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 59.4 ∘C.