A chunk of 0 C ice, mass 145g, is dropped into 75g of water at 62 C. The heat of the fusion of water is 335J/g. What is the result after thermal equlibrium is attained?

I would check to see how much heat is required to change T of H2O from 62 to zero. mass H2O x specific heat water x delta T.

Then see if you have that much heat from melting the ice.
mass ice x heat fusion = ??
I thin you will have ice left over with ice at zero and water at zero. You figure how much ice is left. Post your work if you get stuck.

To find the result after thermal equilibrium is attained, we need to calculate the total heat gained and lost during the process.

The heat gained by the ice to reach its melting point can be calculated using the formula:

Q1 = mass of the ice * heat of fusion of water

Substituting the given values, we get:

Q1 = 145g * 335J/g = 48575J

The heat lost by the water to reach the melting point can be calculated using the formula:

Q2 = mass of the water * specific heat capacity of water * (temperature change)

Since the water is initially at 62°C and needs to reach the melting point (0°C), the temperature change is:

Temperature change = 62°C - 0°C = 62°C

Using the specific heat capacity of water, which is 4.18J/(g°C), we can calculate Q2:

Q2 = 75g * 4.18J/(g°C) * 62°C = 19317J

Now that we have calculated the heat gained by the ice and the heat lost by the water, we can determine the result after thermal equilibrium is attained.

Since heat is conserved in a closed system, the heat gained by the ice (Q1) will be equal to the heat lost by the water (Q2). Therefore:

Q1 = Q2

48575J = 19317J

To find the final temperature of the system, we assume that the ice completely melts and that the resulting mixture reaches the same final temperature. In this case, the final temperature will be 0°C.

So, after thermal equilibrium is attained, the final result will be a mixture of melted ice at 0°C and water at 0°C.