During the summer after your first year at Carnegie Mellon, you are lucky enough to get a job making coffee at Starbucks, but you tell your parents and friends that you have secured a lucrative position as a "java engineer." An eccentric chemistry professor (not mentioning any names) stops in every day and orders 200ml of Sumatran coffee at precisely 60.0°C. You then need to add enough milk at 1.00°C to drop the temperature of the coffee, initially at 95.0°C, to the ordered temperature. Calculate the amount of milk (in ml) you must add to reach this temperature. Show all your work in the provided spaces.

In order to simplify the calculations, you will start by assuming that milk and coffee have the specific heat and density as if water. In the following parts, you will remove these simplifications. Solve now this problem assuming the density is 1.000 g/ml for milk and coffee and their specific heat capacity is 4.184 J/(g ºC).

How many ml of milk is required to drop the temp 60 degrees celsius, if confused the coffee when made fresh is 95 degrees celsius and needs to be lowered to 60 degrees celcius