# An object with a mass of 1 kg, temperature of 320 ^oC, and a specific heat of 14 J/(kg*K) is dropped into a container with 16 L  of water at 0^oC . Does the water evaporate? If not, by how much does the water's temperature change?

Feb 14, 2018

The water does not evaporate and the change in temperature is $= {0.07}^{\circ} C$

#### Explanation:

The heat is transferred from the hot object to the cold water.

Let $T =$ final temperature of the object and the water

For the cold water, $\Delta {T}_{w} = T - 0 = T$

For the object $\Delta {T}_{o} = 320 - T$

${m}_{o} {C}_{o} \left(\Delta {T}_{o}\right) = {m}_{w} {C}_{w} \left(\Delta {T}_{w}\right)$

The specific heat of water is ${C}_{w} = 4.186 k J k {g}^{-} 1 {K}^{-} 1$

The specific heat of the object is ${C}_{o} = 0.014 k J k {g}^{-} 1 {K}^{-} 1$

The mass of the object is ${m}_{0} = 1 k g$

The volume of water is $V = 16 L$

The density of water is $\rho = 1 k g {L}^{-} 1$

The mass of the water is ${m}_{w} = \rho V = 16 k g$

$1 \cdot 0.014 \cdot \left(320 - T\right) = 16 \cdot 4.186 \cdot T$

$320 - T = \frac{16 \cdot 4.186}{1 \cdot 0.014} \cdot T$

$320 - T = 4784 T$

$4785 T = 320$

$T = \frac{320}{4785} = {0.07}^{\circ} C$

As the final temperature is $T < {100}^{\circ} C$, the water will not evaporate