To find the molarity of the urea solution, we will follow these steps:

1. Calculate the number of moles of urea using its molecular weight.

2. Determine the volume of the solution using its mass and density.

3. Use the number of moles and volume of the solution to calculate the molarity.

Step 1: Calculate the number of moles of urea.

The number of moles of a substance $ n $ is determined by dividing the mass of the substance ($ m $) by its molecular weight ($ M $):

$ n = \frac{m}{M} $

For urea, $ m = 120 \text{ g} $ and $ M = 60 \text{ g/mol} $, thus:

$ n_{urea} = \frac{120 \text{ g}}{60 \text{ g/mol}} $

$ n_{urea} = 2 \text{ moles} $

Step 2: Determine the volume of the solution.

The volume $ V $ of the solution can be found by dividing the mass of the solution by its density $ \rho $:

$ V = \frac{mass_{solution}}{\rho} $

The mass of the solution is the sum of the mass of urea and the mass of water. Thus:

$ mass_{solution} = mass_{urea} + mass_{water} = 120 \text{ g} + 1000 \text{ g} $

$ mass_{solution} = 1120 \text{ g} $

The density of the solution $ \rho $ is given as 1.15 g/mL. Therefore, the volume in milliliters (which is equivalent to cubic centimeters) is:

$ V = \frac{1120 \text{ g}}{1.15 \text{ g/mL}} $

$ V = 973.91 \text{ mL} $

To convert milliliters to liters (since molarity is defined in terms of liters), we divide by 1000:

$ V = 0.97391 \text{ L} $

Step 3: Calculate the molarity.

Molarity ($ M $) is defined as the number of moles of solute divided by the volume of solution in liters:

$ M = \frac{n_{solute}}{V_{solution}} $

$ M = \frac{2 \text{ moles}}{0.97391 \text{ L}} $

$ M \approx 2.05 \text{ M} $

Therefore, the molarity of the urea solution is approximately 2.05 M, which corresponds to Option C.