Question

(a) How much heat transfer (in kJ) is necessary to raise the temperature of a 0.150 kg piece of ice from -22.0°C to 126°C, including the energy needed for phase changes? (Assume the substance remains at a constant volume throughout each stage of the heating process.) kJ (b) How much time (in s) is required for each stage, assuming a constant 21.0 kJ/s rate of heat transfer? (Enter your answers as a comma-separated list. Enter your times in order from the earliest stage to the final stage of the heating process.) t = S

Answer 1

mass of ice 0.15 kg = 150g Initial temperature of ice = 2900 Final temperature = 186°C 1. Ice temperature is raised from -29°c to 0°C g. Ice at 0°C is converted to 0°C water 3. water at o'c is converted to water at 100°C 4. water at 100°c is converted to steam at 100°C. 5. u4 steam at 100°C is converted to steam at 126°C Q - 150 x (V2) (29) = 1650 cal = 150 x 80 = 19000 cal Q3 = 150 X (1) (100) = 15000 cal Qy = 1504 540 Q4 150 x(YA)(26) = 1950 cal 81000 cal Qg

Q- Q + Qg + Q₃ + Qu + Qs ng 111 600 cal - 4.67X105 J = 4670 16 kJ b) heat transfer rate 21 kJ/s P = 5016-72 cal/8 ti = Q, 0.33 sec P 2.39 2 sec tg = A2 t3 = 23 2.99 sec P 16.146 sec = ty 0.39 sec ts = = Q5 Р

please rate it up thanks :)