An insulated beaker with negligible mass contains liquid water with a mass of 0.350 kg and a temperature of 69.7degrees C.
How much ice at a temperature of -17.5degrees C must be dropped into the water so that the final temperature of the system will be 33.0 degrees C?
Take the specific heat of liquid water to be 4190 J/kgkelvin, the specific heat of ice to be 2100J/kgkelvin , and the heat of fusion for water to be 334 kJ/kg.
The Attempt at a Solution
i think i am supposed to calculate the heat it takes for the 69.7 degree water to reach 33 degrees. and set that equal to the mcdeltaT equation for the ice and solve for mass of the ice. but i keep getting the answer wrong and it isnt my units. also how do i take into account the phase change from ice to water, do i just add it to the mcdeltaT equation for ice? any advice is appreciated