Since we know the heat of fusion of water on a per mass basis, we can calculate the heat required to melt 2kg of ice:

Ice melts at a constant temperature of .

Now, use the equation for entropy:

Recall that in an isothermal process, the change in internal energy of the has is 0. Thus, we can make use of the following equation to calculate the work done.

Since the change in internal energy is 0, we can rewrite the equation as:

In other words, in order to maintain a constant internal energy of the system, the gas must do the same amount of work on its surrounding as the amount of energy it absorbs from the surroundings in the form of heat.

In order to find out which of the answer choices is not one of the laws of thermodynamics, we'll need to consider each one.

The zeroth law of thermodynamics says that if two systems are in each in thermal equilibrium, respectively, with a third system, then they must be in thermal equilibrium with each other.

The first law of thermodynamics says that energy can only be converted from one form to another and cannot be created.

The second law of thermodynamics says that all spontaneous processes must lead to an increase of entropy in the universe.

The third law of thermodynamics says that at a temperature of absolute zero, all motion within a system ceases.

The only other answer choice left states that energy and mass are interconvertible. Although this is a true statement, as is stated by Einstein's famous equation , this is not a thermodynamic law.

We can use the 1st law of thermodynamics to solve this problem:

We are given the heat applied to the system, so we need to calculate the work done by the system. Since we were told that this is isobaric expansion, we can use the following expression for work:

Substituting this in, we get:

Plugging in values, we get:

We will begin with the 1st law of thermodynamics:

We know that there is no change in internal energy, so we can say:

Also, the problem statement tells us that this is isothermal expansion, we can use the following expression for work:

Plugging this into our expression, we get:

Rearranging for the change in volume, we get:

We have all of these values, so time to plug and chug:

In an isothermal process, there are two possibilities: the gas is expanding or the gas is being compressed. If the gas is expanding, the gas is doing work and therefore needs heat in order to remain at constant temperature (which is the definition of an isothermal process). If the gas is compressed, then work is being done on the gas and heat must be emitted in order for the temperature to remain constant. We're told heat is added, so the gas must be expanding. This means the volume is increasing and work is being done by the gas. Therefore, those two choices are not the answer. The pressure must decrease, which can be seen using the formula . Since temperature is constant, if volume goes up, pressure must go down. The average kinetic energy (A.K.A. temperature) will remain constant. Work is not being done on the gas, so that is the correct answer.

Both of these conceptual methods of figuring out if heat must be added or released can be mathematically computed using the formula .  is the heat added to the gas,  denotes the work done by the gas, and  denotes the change in internal energy, which is directly related to temperature.

Here, we need to use the first law of thermodynamics:

Since the heat is added to the system, the sign is positive. Moreover, the work can be calculated using:

Now, we can simply add these two parts to get the change in internal energy.