Question

An eager scientist on a hot summer day needs to determine how much ice to buy. She has a cooler which is filled with 34 cans of soda at a temperature of 84.1 ∘ F. Each can has a mass of 411 g. The scientist wants the temperature of the drinks to be 40.8 ∘ F. If there is no heat lost by the cooler and ignoring any heat lost to the soda containers, what mass m ice of ice needs must she add to her cooler? Assume the temperature of the ice is 32.0 °F.

Answer 1

There will be no heat loss to the surrounding the net heat is zero.. Oneto heat needed for a bhase change. Q = tmL heat needed for a temperature change it, Q=MCAT The ice has to melt to liquid water- absorb heat a tmas ef= 3.34X10ST/19 Heat needed to for the ice is- Dice = micelf & Mice Cwater (T- Tice) Cwater = 4190 I / lyk, O soda = msoda Csoda (T- Tsoda ) Closed system, Onat 20 Dice +34 Osoda 0 Dice =-34 Dean Mice (ust water (T-Tice)) =-34m soda sodd T-Tsoda, - 34m soda Csoda (T- Isada) 2ft Cwator (T- Tice) =-34(0.411kg) 4290/278.038-302.09) 3.34X10% + 419012785038-233.15) - + 1408270.095 354480.72 I Mice = 3.97 kg Mice - - Tsoda = 84. 1f=302.094 K Tice = 32 f = 273.15K T = 40.8 f= 2781038k