1 m of carbon monoxide at a pressure of 1 N/mm² and temperature 300°C, expands 10 times its original volume and its final temperature will be 25°C. Calculate (i) mass (i) change in entropy by considering temperature, volume, entropy relationship (iii) change in entropy by considering temperature, pressure, entropy relationship (iii) change in entropy by considering pressure, volume, entropy relationship.
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- The standard enthalpies of formation, at 25.00 oC, of methanol (CH4O(l)), water (H2O(l)), and carbon dioxide (CO2(g)) are respectively -238.7 kJ/mol, - 285.8 kJ/mol, and -393.5 kJ/mol. Calculate the change in surrounding entropy (in J/K) when burning 13.6 g of methanol under a constant pressure of 1.000 atm at 25.00 oC (N.B., combustion is the reaction of a substance with oxygen molecule to produce water and carbon dioxide).A closed, but not isolated system is in thermal contact with its surroundings. The system's volume is fixed at 7.3 L. Both the system and surrounds have a temperature of 25 °C. A chemical reaction occurs inside the system for which ΔrU = 11.38 KJ. (A) What is the change in entropy for the surroundings for the process, ΔSsurr? (B) What are the ranges of possible values for the change in entropy of the system, ΔSsys , for this process?The standard enthalpies of formation, at 25.00 oC, of methanol (CH4O(l)), water (H2O(l)), and carbon dioxide (CO2(g)) are, respectively, -238.7 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol. Calculate the change in the entropy of the surroundings (in J/K) upon the combustion of 13.3 g of methanol under a constant pressure of 1.000 atm and a temperature of 25.00 oC. N.B. combustion is the reaction of this substance with molecular oxygen to produce water and carbon dioxide.
- The enthalpy of vaporization (deltaHvap) of water was experimentally determined to be 151.3 kJ for 3.72 mols of water at 100 degrees Celsius? Calculate the molar entropy of vaporaization (deltaSvap,m) of water.Describe how to find the relationshipbetween the state properties (P, V, T ) of agas and its molar mass or density.Suppose a certain small bird has a mass of 30 g. What is the minimum mass of glucose that it must consume to fly to a branch 10 m above the ground? The change in Gibbs energy that accompanies the oxidation of 1.0 mol C6H12O6(s) to carbon dioxide and water vapour at 25 °C is -2828 kJ.
- An ideal gas (0.487 mol) at 250 K and 1.5 bar is compressed to 5.7 bar.(a) Calculate the change in Gibbs free energy, ΔG (in kJ).The change in Gibbs energy that accompanies the combustion of C6H12O6(s) to carbon dioxide and water vapour at 25 °c is -2828 kJ mol-1. The potential energy of an object of mass m at a height h, relative to that at the Earth's surface is given by mgh, where g = 9.81 m s-2 is the acceleration of freefall. How much glucose does a person of mass 65 kg need to consume to climb through 10m?Pure water under the atmospheric pressure of 100,000 Pa is converted to steam at a temperature of 100 0C. What statement can you make regarding the relation between Gibbs free energy (or chemical potential) of water and steam at 100 0C, under atmospheric pressure. If the heat needed to vaporise 1 kg of water to steam at 100 0C is 2265 kJ/kg. Work out the difference between entropy of steam and water at the boiling temperature. b) If a small amount of salt 0.0002 mol is added to every 18 g of water, calculate the chemical potential change of water in the salt solution. c) Assuming that the chemical potential of water in the solution does not change much with pressure, work out the pressure at which the water in the salt solution will boil, at 100 0 You may take steam as being an ideal gas.
- 1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure. a) Calculate entropy change of the system, surrounding and universe. (temperature of the environment is -10 °C) b) Make some comments on entropy changes from the obtained data Please use the following data for water : Melting entalpy of ice (ΔHmelting) at 0°C and 1 bar is 6020 J mol-1. Cp (H2O (s)) = 37,7 J mol-1 K-1 Cp (H2O (l)) = 75,3 J mol-1 K-1A student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = JP3B.7 A block of copper of mass 500 g and initially at 293K is in thermalcontact with an electric heater of resistance 1.00 kΩ and negligible mass. Acurrent of 1.00A is passed for 15.0 s. Calculate the change in entropy of thecopper, taking Cp,m = 24.4 JK−1mol−1. The experiment is then repeated with thecopper immersed in a stream of water that maintains the temperature of thecopper block at 293K. Calculate the change in entropy of the copper and thewater in this case.P3B.8 A block of copper (Cp,m = 24.44 JK−1mol−1) of mass 2.00 kg and at0 °C is introduced into an insulated container in which there is 1.00molH2O(g) at 100 °C and 1.00 atm. Assuming that all the vapour is condensed toliquid water, determine: (a) the final temperature of the system; (b) the heattransferred to the copper block; and (c) the entropy change of the water, thecopper block, and the total system. The data needed are given in ExerciseE3B.7a.