What is the change in entropy when 2.00 kg of water at 100°C is heated to...
What is the change in entropy of 100 g of water when it is heated from room temperature (20 °C) to body temperature (37 °C)? Use p.m-75.5 J K i mol l
Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of water is heated from 80.00 °C to 110.0 °C at 1 atm pressure. Molar Heat Capacity H20(I) = 75.3 JK' molt H20(9) = 36.4 JK' moi Enthalpy of Vaporization at 100 °C = 40.7 kJ moi? -1 Answer:
Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of water is heated from 10.00°C to 300.0 °C at 1 atm pressure. Molar Heat Capacity H2O(1) = 75.3 JK' moi? H2O(g) = 36.4 JK' mol Enthalpy of Vaporization at 100 °C = 40.7 kJ mol .-1 -1 Answer:
What is the generated entropy (in kJ/K) when 1 kg of liquid water at 25°C is heated to saturated vapor at 100°C in an oven that is at 150°C. Hint: the effect of pressure on the entropy of liquids or solids is usually negligible. Now assume you are trying to heat 1 kg of liquid water at 25°C to saturated vapor at 100°C, but you want to do it in an oven that is at 80°C. This is obviously impossible...
5.00 kg of liquid water at 100 kPa is heated from 20 C to 80 C on the stove. Neglecting evaporation of the water, determine the entropy change of the water. Assume cv= 4.20 kJ/(kg-K)
What is the entropy change of the universe (in J K-1)when 2.00 mol of liquid water at 0 °C freezes in a freezer compartment whose temperature is -15 °C? Assume the freezer is a perfect insulator. (AHfus = 6.01 kJ mol-1 for water) Select one: O a. +90.6 O b. +46.6 C. -2.6 O d. -44.0 o e. +2.6
1. a) Calculate the change in entropy (AS) when one mole of diamond is heated from a temperature of 0 K to 400 K at a constant pressure of 1 bar. The temperature-dependent heat capacity of diamond is C 2.9x10 T J/(mol K), where T is the absolute temperature in K. b) Given that the entropy of diamond is zero at 0 K, calculate its absolute molar entropy (S) at 400 K from the above result.
Physical Chemistry Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol K1 and 31.75 J mol K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g1. The molar mass of aluminum is...
A cylinder made of brass with a mass of 0.80 kg is heated to 850°C, then dropped into 5.00 kg of water at 11°C. What is the total change in entropy (in J/K) of the cylinder-water system, assuming no energy is lost by heat from this system to the surroundings? The specific heat of brass is 380 J/(kg · K), and the specific heat of water is 4,186 J/(kg · K). (Hint: note that dQ = mcdT.)
A rod made of cobalt with a mass of 0.80 kg is heated to 850°C, then dropped into 7.00 kg of water at 10°C. What is the total change in entropy (in J/K) of the rod-water system, assuming no energy is lost by heat from this system to the surroundings? The specific heat of cobalt is 420 J/(kg · K), and the specific heat of water is 4,186 J/(kg · K). (Hint: note that dQ = mcdT.)