20 grams of ice initially at -15◦C is placed on top of 100 grams of 350◦C solid gold in a thermally insulating container. a) What is the change in entropy of the gold bar? a (°℃−¹)MaterialGoldCopperAluminum1.65×10-52.3x10-5Stainless Steel 1.75×10-5WaterEthyl AlcoholIce1 atm = 1.01×105 PaNA = 6.022×102³ particles/molR = 8.3145 J/(mol K)kB = 1.38×10-23 J/Ko = 5.67 × 10-8W/(m²K4)c (J/(kg K)) C (J/(mol K)) | Lf (J/kg) Lv (J/kg) density (kg/m³)1292519,3008,9602,7007,5004190751,0003.33×105 22.6×1051.09×105 8.79×1052400110790209037.6917

Answered: Image /qna-images/answer/20c77ede-8551-4256-b52c-7874fcb15a70.jpg

Answered: 20 grams of ice initially at -15◦C is…

Similar questions

A system consists of a 1.2 kg block of copper at 20∘C and 1.5 kg block of copper at 200 ∘C. The two blocks, isolated from the environment, are placed in contact until thermal equilibrium is reached. The specific heat of copper is 385 J/kg⋅K. What is the change in entropy of the system?
The difference in entropy AS=Sg-SA for two states A and B of a system can be computed by AS=[dQ/T provided: O a. A andB are on the same adiabat. O b. A and B have the same temperature. O c. The energy absorbed as heat by the system is first computed O d. A reversible path is used for the integral
What is the entropy change for 3.20 mol of an ideal monatomic gas undergoing a reversible increase in temperature from 380 K to 425 K at constant volume?
Suppose you put a cube of ice of mass 100 g into a glass of water at just above 0°C. When the ice melts, about 33 kJ of energy is absorbed from the surroundings as heat. What is the change in entropy of (a) the sample (the ice) and (b) the surroundings (the glass of water)?
A parcel is lifted adiabatically from z = 0 to z = H. What is the change in entropy?
30 grams of ice at -5 Celsius melt while being left at room temperature of 28 Celsius. After melting its temperature rises to 28 Celsius. Determine the total change of entropy of the ice. [Cice = .5 cal/g.C, Lf = 79.6 cal/gram] 1 calorie = 4.184 J Options: A. 49.97 J/K B. 34.68 J/K C. 53.11 J/K D. 38.27 J/K E. 44.22 J/K
What is the entropy change when 0.50 moles of CHCl₃ vaporizes at 61.0 °C? [∆H(vap) = 29.6 kJ/mol at 61.0 °C] ____J/K