An object with a mass of $3 kg$ , temperature of $173 ^oC$ , and a specific heat of $23 J/(kg*K)$ is dropped into a container with $32 L$ of water at $0^oC$ . Does the water evaporate? If not, by how much does the water's temperature change?

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Answer 1 · 2017-07-25T14:21:35

The water does not evaporate and the change in temperature is $=0.09^@C$

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 $DeltaT_o=173-T$

$m_o C_o (DeltaT_o) = m_w C_w (DeltaT_w)$

$C_w=4.186kJkg^-1K^-1$

$C_o=0.023kJkg^-1K^-1$

$3*0.023*(173-T)=32*4.186*T$

$173-T=(32*4.186)/(3*0.023)*T$

$173-T=1941.3T$

$1942.3T=173$

$T=173/1942.3=0.09^@C$

As $T<100^@C$ , the water does not evaporate

An object with a mass of 3 kg3 kg, temperature of 173 ^oC173 ^oC, and a specific heat of 23 J/(kg*K)23 J/(kg*K) is dropped into a container with 32 L 32 L of water at 0^oC 0^oC . Does the water evaporate? If not, by how much does the water's temperature change?