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.
i keep coming up withthe wrong answer for this
i am getting 1822.111
-713.6=28.2(.385)(Tf-93.8)
i am getting 1822.111
but when i punch it back into the equation its wrong
please help
I don't get 1822.11 no matter how I do it. First, are you using 28.2 g for the metal? The problem states 48.2 g
-713.6 = 48.2*0.385(Tf-93.8) and I get something like 55.3 C. If I check that number, I get this.
q = mass x sp. h. x (Tf-Ti)
q = 48.2 x 0.385 x (55.3-93.8)
q = 48.2 x 0.385 x (-38.5)
q = -714.4 (the small difference is caused by rounding the final T to three s.f. My calculator reads 55.345 and that rounds to 55.3 to 3 s.f. If I used 55.345 I get
q = 48.2*0.385*(55.345-93.8)
q = 48.2*0.385*(-38.455) = -713.61 which is very close.
To determine the final temperature when 713.6 J is released from a 48.2 g sample of copper initially at 93.8°C, you can use the equation:
q = m * c * ΔT
Where:
q = heat energy released (in J)
m = mass of the sample (in g)
c = specific heat capacity of copper (in J/g-°C)
ΔT = change in temperature (final temperature - initial temperature)
In this case, you need to solve for the final temperature (Tf). Rearranging the equation, you have:
ΔT = Tf - 93.8
Now substitute the given values into the equation:
713.6 J = 48.2 g * 0.385 J/g-°C * (Tf - 93.8°C)
Next, let's solve for (Tf - 93.8):
(Tf - 93.8) = 713.6 J / (48.2 g * 0.385 J/g-°C)
(Tf - 93.8) = 36.13 °C
Now, solve for Tf by adding 93.8 to both sides of the equation:
Tf = 36.13 + 93.8
Tf = 129.93°C
Therefore, the final temperature of the copper sample is approximately 129.93°C.