What is the final temperature when 1.16 kJ of energy is added to 11.0 g ice at 0°C? Assuming the specific heat of ice is 2.03 J/g * C.
the heat of fusion for ice/water is 332 J/g * C
looks like the ice partially melts , so the temperature doesn't change
To find the final temperature when energy is added to ice, we can use the formula:
q = m * c * ΔT
Where:
q is the energy transferred (in Joules)
m is the mass of the substance (in grams)
c is the specific heat capacity of the substance (in J/g * °C)
ΔT is the change in temperature (in °C)
In this case, we are given:
q = 1.16 kJ = 1160 J (since 1 kJ = 1000 J)
m = 11.0 g
c = 2.03 J/g * °C
ΔT = ? (final temperature that we need to find)
Rearranging the formula to solve for ΔT:
ΔT = q / (m * c)
Substituting the given values:
ΔT = 1160 J / (11.0 g * 2.03 J/g * °C)
Now we can calculate ΔT.