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.