If 309 J of heat are removed from 10.0 g of ice (specific heat = 2.06 J/g
ºC) at -5.5 ºC, what is the final temperature of the ice sample?
-q = mass ice x specific heat ice x (Tfinal=Tinitial)
-309 = 10.0 x 2.06 x [Tf -(-5.5)]
Solve for Tf.
Thank you Dr. Bob
-20.5
Well, let me calculate that for you. To find the final temperature, we can use the formula:
Q = m * c * ΔT
Where:
Q is the amount of heat
m is the mass of the ice
c is the specific heat of the ice
ΔT is the change in temperature
In this case, Q = -309 J, m = 10.0 g, c = 2.06 J/g ºC, and the initial temperature is -5.5 ºC. We want to find ΔT, so we can rearrange the formula as:
ΔT = Q / (m * c)
Substituting in the values, we get:
ΔT = -309 J / (10.0 g * 2.06 J/g ºC)
Calculating that, we find:
ΔT = -309 J / 20.6 J/ºC
ΔT ≈ -15 ºC
So the final temperature of the ice sample should be -5.5 ºC - 15 ºC = -20.5 ºC. Well, that's a chilling temperature!
To find the final temperature of the ice sample, we need to use the equation:
Q = m * c * ΔT
where Q is the heat transfer, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.
In this case, the heat transfer (Q) is -309 J because heat is being removed from the ice. The mass (m) is 10.0 g, and the specific heat capacity (c) is 2.06 J/g ºC.
We need to find the change in temperature (ΔT). The initial temperature of the ice sample is -5.5 ºC, and we want to find the final temperature. So, ΔT = final temperature - initial temperature.
Rearranging the equation, we have:
ΔT = Q / (m * c)
Plugging in the known values, we get:
ΔT = -309 J / (10.0 g * 2.06 J/g ºC) ≈ -15 ºC
Now, to find the final temperature, we can rearrange the equation again:
final temperature = initial temperature + ΔT
Plugging in the known values, we get:
final temperature = -5.5 ºC + (-15 ºC) = -20.5 ºC
Therefore, the final temperature of the ice sample is approximately -20.5 ºC.