# An object with a mass of #4 kg#, temperature of #240 ^oC#, and a specific heat of #15 J/(kg*K)# is dropped into a container with #15L # of water at #0^oC #. Does the water evaporate? If not, by how much does the water's temperature change?

##### 1 Answer

#### Answer:

The object does not vaporise the water. It causes a temperature change of

#### Explanation:

Evaporation of a liquid can occur at any temperature. So we could say "Yes" in answer to the question "Does the water evaporate?" However, let’s assume the question meant "Does all of the water get vaporised?" (I.e. is the water raised to its boiling point and then boiled away?)

To answer the question I will structure my solution as follows:

- Calculate the energy required to raise the temperature of the water to 100ºC.
- Calculate the energy required to completely vaporise the water.
- Calculate the energy available for transfer from the object and compare that value to energies 1 and 2 above.
- If the object does not have enough energy to vaporise the water the temperature change in the water will be calculated.

**Some preliminary data and calculations.**

Conversion of the volume of water into m³:

#V = 15 L = 15 × 10^(-3) m^3#

Calculation of the mass of water:

#m_w = ρV = 1000 × 15 × 10^(-3) = 15 kg#

Specific heat capacity of water:

#c_w = 4200 J.kg^(-1).K^(-1)#

Latent heat of vaporisation of water:

#L_(v(water)) = 334 kJ.kg^(-1)#

**An initial note about the question.**

As you can see from the data that was provided the object has both a *much* smaller specific heat capacity and a smaller mass than the water.

So we can provisionally tell that the impact of the object on the water is going to be very small indeed. It is in fact so small that I wonder whether some of the data provided was incorrect?

**1. Energy required to increase temperature of water to boiling point.**

#DeltaQ_1 = m_wc_wDeltaθ = 15 × 4200 × (100 - 0)#

#⇒ DeltaQ_1 = 6.3 MJ#

**2. Energy required to vaporise all of the water.**

#DeltaQ_2 = m_wL_(v(water)) = 15 × 334 × 10^3#

#⇒ DeltaQ_2 = 5.0 MJ#

**3. Energy available from the 4kg object.**

The lowest temperature the object could fall to and successfully vaporise the water would be

Data for the object:

#DeltaQ_3 = m_oc_oDeltaθ = 4 × 15 × (240 - 100) = 8400 J#

Compare the energies. We can see that 8400 J is much less than 6.4 MJ (

We don’t even need to consider comparing 8400 J with the energy required to vaporise the water (calculated in part 2).

**4. By how much does the water’s temperature change?**

Since we know the water does not undergo a phase change we will only need to use the specific heat capacity equation for both the object and the water.

I will define the final temperature of the water as

Object starts at

Water starts at

Assuming that all heat energy transferred by the object is absorbed by the water we can state the following:

#DeltaQ_w = DeltaQ_o#

#⇒ m_wc_wDeltaθ_w = m_oc_oDeltaθ_o# ①

Noting the above information about the temperature changes we can further define the ∆θ terms:

#Deltaθ_w = θ_x – 0#

#Deltaθ_o = 240 – θ_x#

Substitute those into equation ①:

#⇒ m_wc_w(θ_x – 0) = m_oc_o(240 – θ_x)#

#⇒ m_wc_wθ_x = 240m_oc_o – m_oc_oθ_x#

Rearrange for

#⇒ θ_x (m_wc_w + m_oc_o) = 240m_oc_o#

#⇒ θ_x = (240m_oc_o)/(m_wc_w + m_oc_o)#

Now substitute the values into the equation:

#⇒ θ_x = (240 × 4 × 15)/(15 × 4200 + 4 × 15) = 0.23^@"C"#

So the temperature change in the water is