A 271-g sample of nickel at 94.1°C is placed in 100.0 mL of water (density = 1.00 g/mL) at 23.9°C. What is the final temperature of the water?

[Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g·K) and of water = 4.184 J/(g·K).]

heat lost by Ni + heat gained by H2O = 0

[mass Ni x specific heat Ni x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0

Would I have to rearrange the equation to solve for the final temp of the water?

You can but that's the hard way to do it. It is much easier to substitute the individual numbers and work it out by pieces.

Do I already know the final temp of the nickel because I don't know where to start even though you have given me the equation.

No, of course you don't know the final T. That's what you're trying to find. It ways that in the problem, "What is the final T if ..."

heat lost by Ni + heat gained by H2O = 0
[mass Ni x specific heat Ni x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
mass Ni = 271 g
specific heat Ni = 0.444
Tinitial Ni = 94.1 C
Tfinal = ?
mass H2O = 100 mL and since water has density of 1.00 g/mL, this is 100 g.
specific heat H2O = 4.184
Tinitial H2O = 23.9 C
Tfinal = ?
Note: Tfinal for Ni and Tfinal for H2O will be the same T since that is where equilibrium will be attained; i.e., when the Ni has lost heat and the H2O has gained heat and both are at the same final temperature.

Okay. Thanks for clarifying the problem for me.

To solve this problem, we can use the principle of conservation of energy.

First, we need to calculate the heat lost by the nickel and the heat gained by the water.

The heat lost by the nickel can be calculated using the formula:

Q = m * c * ΔT

Where Q is the heat lost, m is the mass of the nickel, c is the specific heat capacity of nickel, and ΔT is the change in temperature.

Q_nickel = (271 g) * (0.444 J/(g·K)) * (94.1°C - Tf)

Next, we need to calculate the heat gained by the water using the formula:

Q = m * c * ΔT

Where Q is the heat gained, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature.

The mass of the water can be calculated using the density formula:

m_water = volume * density

m_water = (100.0 mL) * (1.00 g/mL)

Now, we can calculate the heat gained by the water:

Q_water = (m_water) * (4.184 J/(g·K)) * (Tf - 23.9°C)

Since there is no heat lost or gained to the surroundings, the heat lost by the nickel is equal to the heat gained by the water:

Q_nickel = Q_water

Now we can set up the equation:

(271 g) * (0.444 J/(g·K)) * (94.1°C - Tf) = (m_water) * (4.184 J/(g·K)) * (Tf - 23.9°C)

Simplifying the equation:

(271 g) * (0.444 J/(g·K)) * (94.1°C - Tf) = (100.0 g) * (4.184 J/(g·K)) * (Tf - 23.9°C)

Now we can solve for Tf.