Molar mass of mercury = 200.592 give/mol. No.of moles is equal to 22.3/200.592 = 0.11117 mol,. H = 0.11117. * 28 *(298-234.32) = 198.22 J,. 234.32K liquid to 234.32 K solid then H. =0.11117. * 2.29. = 0.2544 KJ total heat = 0.1982. +0.2544 = 0.4532 KJ.
Calculate the heat energy released when 22.3 g of liquid mercury at 25.00 degree C is...
Calculate the heat energy released when 10.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point.
Calculate the heat energy released when 10.710.7 g of liquid mercury at 25.00° C is converted to solid mercury at its melting point. heat capacity of Hg(l)Hg(l) 28.0 J/(mol·K) melting point 234.32 K enthalpy of fusion 2.29 kJ/mol
Calculate the heat energy released when 17.4 g of liquid mercury at 25.00 degreeC is converted to solid mercury at its melting point.
Question 7 of 10 Calculate the energy released as heat when 17.8 g of liquid mercury at Constants for mercury at 1 atm 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg() 28.0 J/(mol-K) melting point 234.32 K enthalpy of fusion 2.29 kJ/mol kJ q =
n 8 OT IU > AllerPL II Calculate the heat energy released when 25.5 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. Constants for mercury at 1 atm heat capacity of Hg(1) 1 28.0 J/(mol.K) melting point 234.32 K enthalpy of fusion 2.29 kJ/mol 9 = -0.9
1. At 1 atm, how much energy is required to heat 35.0 g H2O(s) at −10.0 ∘C to H2O(g) at 137.0 ∘C? Use the heat transfer constants found in this Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O (steam) 2.000...
Using the provided data, calculate the amount of heat, in kJ, required to warm 22.3 g of solid acetone, initially at -110. °C, to gaseous acetone at 74. °C. acetone molar mass 58.0791 g/mol melting point -95. °C boiling point 56. °C ΔHfus 5.69 kJ/mol ΔHvap at bp 29.1 kJ/mol Cs, solid 1.6 J/g⋅°C Cs, liquid 2.16 J/g⋅°C Cs, gas 1.47 J/g⋅°C
How much heat energy is required to convert 82.0 g of solid ethanol at -114.5 degree C to gaseous ethanol at 167.4 degree C? The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of -114.5 degree C and a normal boiling point of 78.4 degree C. The specific heat capacity of liquid ethanol is 2.45 J/g middot degree C and that of gaseous ethanol...
2. Solid mercury at -89 °C is added to liquid water at 0°C. When the system reaches thermal equilibrium all the water is ice and half of the original mercury is liquid. Assume that no heat is lost to the surroundings and find the ratio of the mass of mercury to the mass of water (mHg/m1,0). Melting Point Heat of Fusion Heat Capacity (solid) (°C) (J/kg) (J/kg.Cº 0.10 x 105 140 3.00 x 105 2000 Mercury Water -39 0
The following information is given for mercury at 1 atm: boiling point-357°C AHvap 0.296 kJ/g melting point--39 °C AHfus 11.6 J/g Heat is added to a sample of solid mercury at its normal melting point of -39 °C. How many grams of mercury will melt if 12.3 kJ of energy are added?