125.0- 100.0- °C 0.0- -25.0- 6010 J 940 J 0 7520 J 10000 AH vaporization liquid gas 20000 30000 Heat added (1) 40000 50000 Heating curve for 1.00 mole of water at 1 atm What is the specific heat for water between 0°C and 100.0°C? 60000
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- As some of you know, I am an aficionado of Starbuck's Steamed Milk, Venti size. Steamed milk is made by passing superheated steam into a stainless steel container containing the milk. Assume that the stcam is at 25C,L-$40 calories/gram, and the specific heat of steam is 0.500 calories/gram/degree C. Also assume that the milk is at 5°C and that 750 ml of milk represent the Venti size. The stainless steel container can be considered to have a mass of 400. grams and a specific heal capacity of 0.600 Jgram/K. If the density of milk is its specific heat is 4.184 Vgram/K, how many grams of steam does it take to raise the milk's temperature to a comfortable 65 C? Thank you for your help!4.38 g of a gas (28.1 g mol–1) was dissolved in liquid water in a calorimeter with a calorimeter constant of 76.0 J K–1. Prior to mixing everything was equilibrated to 21.2 °C. The resulting solution with a mass of 23.4 g was observed to be at a temperature of -6.8 °C and have a specific heat capacity of 4.61 J g–1 K–1. Determine q per mole for this dissolution process. a. -5150 J/mol b. -1.94 × 104 J/mol c. 2.89 × 105 J/mol d. -3.39 × 105 J/mol e. 3.30 × 104 J/molThe formulas give the enthalpy when Coal and Methane react with oxygen:C+O2->CO2+394 kJ/mol, 12 gram C gives 44 gram of CO2+394 kJCH4+ O2->CO2+2H2O+891 kJ/mol, 16 gram CH4gives 44 gram of CO2+891kJ 1-Calculate the heating value of Coal and Methane in MJ/kg and in kWh/kg.Calculate the lower heating value for Methane. 2-Calculate the amount of CO2 which is produced per kWh for Coal and Methane
- Find ΔS for the system, surroundings, and universe when 28.2 g of liquid H2O is evapourated at 100.0 oC, if the heat required is provided by a hot plate whose temperature is 329 oC. For water, ΔHvap is 40.79 kJ/mol. a. ΔSsystem? b. ΔSsurroundings? c. ΔSuniverse?1. Calculate the standard enthalpy of formation of C10H10. Its standard enthalpy of combustion is shown by the equation: 2C10H10 (l) + 25O2 (g) → 20CO2 (g) + 10H2O (l) ∆H = 10,314 KJ/mol The standard heat of formation (KJ/mol) at 298.15oC : CO2 = -393.5 ; H2O(l) = -285.8 2. Determine ΔG° at 298.15K for the reaction: 4Fe (s) + 3O2 (g) → 2Fe2O3 (s) Given that ΔH° = -1648 kJ ; ΔS° = -549.3 J/K 3. In the picture, Find the the ∆H°rxn if ∆G°rxn is 420 kJ/mol and ∆S°rxn is -143 J/mol*kSeveral ice cubes (ρi = 0.9167 g/cm3) of total volume Vi = 205 cm3 and temperature 273.15 K (0.000 °C) are put into a thermos containing Vt = 680 cm3 of tea at a temperature of 313.15 K, completely filling the thermos. The lid is then put on the thermos to close it. Assume that the density and the specific heat of the tea is the same as it is for fresh water (ρw = 1.00 g/cm3, c = 4186 J/kgK). a. Calculate the equilibrium temperature TE in K of the final mixture of tea and water. b. Calculate the magnitude of the total heat transferred QT in J from the tea to the ice cubes.
- What mass of water (sweat) is required to cool a body weighing 74.1 kg from an initail temperature of 39.7˚C. to normal body temperature (37.4˚C)? Specific heat capacity of human body is 4.00 J/gC and the enthalpy of evaporation is 44.01 kJ/mol and the molar mass of water (sweat) is 18.016 g/mol.How much heat (kJ) is required to convert 3.12 moles of liquid benzene at 75.1°C to gaseous benzene at 115.1°C? The following information may be useful.b.p = 80.1CCm (liquid benzene) = 136.0 J/ (mol * °C)ΔHvap = 30.72 kJ/molCm (gaseous benzene) = 36.6 J/ (mol * °C)12) Between 0 °C and 100 °C, the heat capacity of Hg(l) is given by: Cp,m (Hg, l) [units: J mol-1 K-1] = 30.093 – 4.944 x 10-3T Calculate ΔH and ΔS if the temperature of 1.75 moles of Hg(l) is raised from 0.00 °C to 100.00 °C at constant P.
- Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°C Specific heat capacity (liquid): 2.161 J/g°C Specific heat capacity (gas): 1.291 J/g°C A 791.0 g sample of acetone sitting in the lab has a temperature of 21.7°C. How much heat would be involved in lowering the temperature of the acetone to -200.0°C? (answer in Joules)Under a constant pressure of 1.00 atm, at 25.00oC, the combustion of 1.136 g of C6H12O3(l) raises the temperature of 2.000 kg of water by 2.617 degrees Celsius. Combustion is the reaction of a substance with O2(g) to give CO2(g) and H2O(l). The specific heat capacity of water is 4.184 J K-1 g-1. Ignore the heat capacities of any containers.With the help of the data above, find the values of ΔH, ΔU, Q, and W for the combustion of 1.000 mol of C6H12O3(l) in a steel container of constant volume at 25.00oC.The following formulas give the enthalpy, when Coal and Methane react with oxygen: C+O2->CO2+394 kJ/mol, 12 gram C gives 44 gram of CO2+394 kJ CH4+ O2->CO2+2H2O+891 kJ/mol, 16 gram CH4 gives 44 gram of CO2+891kJ a) Calculate the heating value of Coal and Methane in MJ/kg and in kWh/kg. b) Calculate the amount of CO2 which is produced per kWh for Coal and Methane. Give it in kg/kWh.