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- 6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of transition from white P to red P, , is . The densities of white and red phosphorus are and , respectively. At what temperature does white phosphorus become the stable phase at of pressure? Assume the formula for phosphorus is .To vaporize 100.0 g carbon tetrachloride at its normal boiling point, 349.9 K, and P =1 atm, 19.5 kJ of heat is required. Calculate DHvap for CCl4 and compare it with DU for the same process.Calculate the enthalpy of vaporization for CH3CH2OCH2CH3 (diethyl ether) inkj/mol.GivenAt 00C vapor pressure is 530 mm Hg and it boils at 28 0C.(show your work)
- 2. All liquids have characteristic vapor pressure that vary with temperature. The characteristic vapor pressure for pure water at 22°C is 19.827 mm Hg and at 30.0°C is 31.824 mm Hg. Use these data to calculate the change in enthalphy per mole for the vaporizationSuppose 50.0 g of superheated Na(s) melts at 500 K and 1 bar pressure. Find the ΔSsys, ΔSsurr, and \ΔSuniv in J/K and round the answer to the hundredths place. Thermodynamic Data for Sodium Property Value Tfus 371 K ΔfusH0 at T_{fus}Tfus 2.60 kJ/mol Cp,m0(l) at 298 K 32.7 J K-1 mol-1 Cp,m0(s) at 298 K 28.2 J K-1 mol-1 Assume heat capacities are independent of temperature.a copper container of mass 500 g and contains 1 litre of water at293 K. Prove that the quantity of heat which can be obtained will be ableto raise the temperature of the water in the container to a boiling pointif there are no heat losses. Assume that the specific heat capacity ofcopper is 390 J/(kg K), the specific heat capacity of water is 4.2 kJ/(kg K)and 1 litre of water has a mass of 1 kg.
- 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°CSpecific heat capacity (liquid): 2.161 J/g°CSpecific heat capacity (gas): 1.291 J/g°C How much heat is involved in taking 165.2 g of acetone from 14.7°C to 52.1°C?A glass of water with a mass of 0.32 kg at 20 ° C to be cooled to 0 ° C by dropping ice cubes at 0 °C into it. The latent heat of fusion of ice is 334 kJ/kg , and the specific heat of water is 4.18 kj/kg degree Celsius. The amount of ice that needs to be added is ?Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00 kcal/mol) was used in household refrigerators. What mass of SO2 must be evaporated to remove as much heat as evaporation of1.00 kg of CCl2F2 (enthalpy of vaporization is 17.4 kJ/mol)?The vaporization reactions for SO2 and CCl2F2 are SO2(l) ⟶ SO2(g) and CCl2 F(l) ⟶ CCl2 F2(g), respectively.
- Calculate the enthalpy of vaporization of SO2 at –25°C if the same at its boiling point (i.e. –10°C) be 5950 cal mol–1. Given for SO2, molar heat capacities in liquid and vapor phase are 206 cal K–1 mol–1 and 9.3 cal K–1 mol–1 respectively.Calculate the heat required to bring 10.0 g CCl2F2 from -29.8 °C as a liquid to the gas phase at 10.0 °C. (molar mass = 120.91 g/mol) Cs (gas) = 0.074 kJ/mol·K ΔHvap = 20.1 kJ/mol ΔHfus = 4.14 kJ/molCalculate the heat required to bring 10.0 g CCl2F2 from -29.8°C as a liquid to the gas phase at 10.0°C. (molar mass = 120.91 g/mol) Cs (gas) = 0.074 kJ/mol·K ΔHvap = 20.1 kJ/mol ΔHfus = 4.14 kJ/mol