Question

An ice cube at 0.00 ∘C with a mass of 21.5 g is placed into 500.0 g of water, initially at 31.0 ∘C, in an insulated container. Part A Assuming that no heat is lost to the surroundings, what is the temperature of the entire water sample after all of the ice has melted?

Answer 1

Answer:The temperature of the entire water sample after all of the ice has melted is  $30.3^0C$

Explanation:

As we know that,  

$Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})$.......(1)

where,

q = heat absorbed or released

$m_1$ = mass of ice = 21.5 g

$m_2$ = mass of water = 500.0 g

$T_{final}$ = final temperature = ?

$T1 =\text {temperature of ice}= 0^oC$

$T_2$ = temperature of water =$31.0^oC$

$c_1$ = specific heat of ice= $2.1J/g^0C$

$c_2$ = specific heat of water = $4.184J/g^0C$

Now put all the given values in equation (1), we get

$21.5\times 2.1\times (T_{final}-0)=-[500.0\times 4.184\times (T_{final}-31.0)]$

$T_{final}=30.3^0C$

Thus the temperature of the entire water sample after all of the ice has melted is  $30.3^0C$