Metal Specific Heat (J/g-C)
Al (s) 0.900
Au(s) 0.129
Cu(s) 0.385
Fe(s) 0.444
Hg(l) 0.139
H2O(l) 4.184
C2H5OH(l) 2.46
Using the above table, determine the final temperature if 713.6J is released from a 48.2g sample of copper initially at 93.8o C.
-q = mass Cu x specific heat Cu x (Tfinal-Tinitial). Solve for Tf
-q=63.54*.385(Tf-93.8)
24.4629(Tf-93.8)
24.46-299-2994.34
.008??
Where did you come up with these weird numbers?
I think I've done this problem above but for Christine. Look above for that post, if you aren't Christine, and you'll see how to do it. Or repost and explain what your problem is. I don't even see the 713.6 in the set up.
To determine the final temperature, we can use the formula:
-q = mass Cu x specific heat Cu x (Tfinal - Tinitial)
We are given the following values:
Mass of copper (m) = 48.2 g
Specific heat of copper (s) = 0.385 J/g-C
Initial temperature of copper (Tinitial) = 93.8oC
Energy released (q) = 713.6 J
Let's substitute the values into the formula:
-713.6 = 48.2 x 0.385 x (Tfinal - 93.8)
Now, we can solve for Tf:
-713.6 = 18.557 x (Tfinal - 93.8)
Divide both sides of the equation by 18.557:
-38.493 = Tf - 93.8
Re-arrange the equation:
Tf = -38.493 + 93.8
Tf = 55.307 oC
Therefore, the final temperature, Tf, is approximately 55.307 oC.