If 9.30 x 10^5 J of energy are transferred to 2.00kg of ice at 0 deg C, what is the final temperature of the system?

To find the final temperature of the system, we can use the specific heat capacity of ice and the heat formula:

Q = m * c * ΔT

Where:
Q is the amount of heat transferred
m is the mass of the substance
c is the specific heat capacity of the substance
ΔT is the change in temperature

In this case, the heat transferred is given as 9.30 x 10^5 J, the mass of ice is 2.00 kg, and the specific heat capacity of ice is 2090 J/kg°C.

Using the formula, we can rearrange it to solve for the change in temperature:

ΔT = Q / (m * c)

Substituting the known values:

ΔT = (9.30 x 10^5 J) / (2.00 kg * 2090 J/kg°C)

Calculating this expression gives us the change in temperature. Since the initial temperature is 0°C, we can find the final temperature by adding the change in temperature to the initial temperature:

Final temperature = 0°C + ΔT

Now, let's calculate the final temperature.

To melt all the ice, the heat input required is

= 6.69*10^6 J

Since less than that amount of heat is supplied, not all of the ice will melt. The final temperature will remain 0 C.