Question #eca79
1 Answer
Explanation:
In order to be able to solve this problem, you need to know the specific heat of silver, which is listed as being equal to
c_"silver" = 0.23"J"/("g K")csilver=0.23Jg K
http://www.engineeringtoolbox.com/specific-heat-metals-d_152.html
Now, the idea here is that a substance's specific heat tells you how much energy must be provided in order to increase the temperature of
In your case, you know that you provide a
The equation that establishes a relationship between heat absorbed and change in temperature looks like this
color(blue)(q = m * c * DeltaT)" "q=m⋅c⋅ΔT , where
So, you need to rearrange this equation and solve for
q = m * c * DeltaT implies DeltaT = q/(m * c)q=m⋅c⋅ΔT⇒ΔT=qm⋅c
Plug in your values to get
DeltaT = (300color(red)(cancel(color(black)("J"))))/(32color(red)(cancel(color(black)("g"))) * 0.23color(red)(cancel(color(black)("J")))/(color(red)(cancel(color(black)("g"))) * "K")) = "40.8 K"
This tells you that the temperature of the sample changed by
DeltaT = T_"final" - T_"initial"
T_"final" = "40.8 K" + "20 K" = "60.8 K"
You need to round this off to one sig fig, the number of sig figs you have for the heat absorbed and for the initial temperature
T_"final" = color(green)("60 K")