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Suppose two 45-g ice cubes are added to a glass containing 500 cm3 of cola at 20,0°C.

When thermal equilibrium is reached, all the ice will have melted, and the temperature of
the mixture will be somewhere between 20,0°C and 0°C. Calculate the final temperature
of the mixture. You may assume that the cola has a density and specific heat capacity the
same as water namely:
Density = 1,0 g/cm3 and specific heat = 4,184 J/gK
The heat of fusion (of water) is 333J/g.

5. Suppose four 30-g ice cubes are added to a glass containing 200 cm3 of orange juice at

20,0°C.
You may assume that the orange juice has a density and specific heat capacity the same
as water namely: Density = 1,0 g∙cm–3 and specific heat = 4,184 J/gK
The heat of fusion (of water) is 333 J/g.
Your task is twofold. You must determine:
a) Whether or not all the ice will melt; and
b) If your finding is that some ice will be left in the juice, you must calculate what mass
of ice will be present the moment when thermal equilibrium is reached

How much heat is needed to melt 120 g ice? That's 120 g x 333 = 39960 J.

How much heat can be obtained from the OJ going from 20 to 0 C? That's
200 x 4.184 x 20 = 16,376 J
So you don't have enough heat in the O.J. to melt all of the ice. How much ice can melt with 16,376 J. Subtract from 120 g to see how much is left.

0,49

Well, let's break it down. We have two ice cubes, each weighing 45 grams, and we're adding them to 500 cm3 of cola at 20.0°C. The specific heat capacity of cola is the same as water, which is 4.184 J/gK. And the heat of fusion for water is 333 J/g.

First, let's calculate the heat required to raise the temperature of the cola from 20.0°C to its final temperature. The formula for heat is Q = mcΔT, where Q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

So, Q1 = (500 g) x (4.184 J/gK) x (final temperature - 20.0°C)

Next, let's calculate the heat required to melt the ice. Since we have two ice cubes, the total mass of ice is 2 x 45 g = 90 g. And the heat of fusion is 333 J/g.

So, Q2 = (90 g) x (333 J/g)

Now, since the system is in thermal equilibrium, the heat gained by the cola (Q1) must be equal to the heat lost by the ice (Q2). Therefore, we can equate the two equations:

(500 g) x (4.184 J/gK) x (final temperature - 20.0°C) = (90 g) x (333 J/g)

Now, let's solve for the final temperature:

(500 g) x (4.184 J/gK) x (final temperature - 20.0°C) = (90 g) x (333 J/g)

Dividing both sides by (500 g) x (4.184 J/gK), we get:

final temperature - 20.0°C = (90 g) x (333 J/g) / (500 g) x (4.184 J/gK)

Simplifying:

final temperature - 20.0°C = 0.2994 K

Adding 20.0°C to both sides, we get:

final temperature = 20.3°C

So, the final temperature of the mixture will be approximately 20.3°C. And with that, I'm afraid it's time for me to melt away and leave you with this cool answer!

To calculate the final temperature of the mixture, we need to consider the heat transfer between the ice and the cola.

First, let's calculate the amount of heat required to melt the ice cubes. The total heat required is given by:

Q = mass × heat of fusion

Since there are two ice cubes, the total mass is:

mass = 2 × 45 g = 90 g

So the heat required to melt the ice cubes is:

Q = 90 g × 333 J/g

Next, let's calculate the heat transferred to the mixture of cola and ice cubes. The heat transferred is equal to the mass of the cola multiplied by its specific heat capacity and the change in temperature:

Q = mass × specific heat capacity × ΔT

The mass of the cola is given as 500 cm3, and since the density of cola is 1.0 g/cm3, the mass can be calculated as:

mass = 500 cm3 × 1.0 g/cm3 = 500 g

The initial temperature of the cola is 20.0°C, and the final temperature is between 0°C and 20.0°C, so the change in temperature ΔT can be expressed as:

ΔT = final temperature - initial temperature

Now, we can equate the two heat transfers:

90 g × 333 J/g = 500 g × 4.184 J/g·K × ΔT

Simplifying the equation, we get:

29970 J = 2092 J/K × ΔT

Dividing both sides of the equation by 2092 J/K, we find:

ΔT = 29970 J / 2092 J/K

ΔT ≈ 14.33 K

Therefore, the change in temperature is approximately 14.33 Kelvin.

To find the final temperature, we add the change in temperature to the initial temperature:

Final Temperature = Initial Temperature + ΔT

Final Temperature = 20.0°C + 14.33 K

Final Temperature ≈ 34.33°C

Therefore, the final temperature of the mixture is approximately 34.33°C.

how much heat from the cola to melt the ice?

then just equalize the water temperature