What amount of heat, in kJ, is required to vaporize 188.15 g of ethanol (C,H OH)? (AHvap = 43.3 kJ/mol) %3D

Calculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Pro

What amount of heat (in kJ) is required to convert 15.5 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･°C; specific heat capacity of liquid = 1.58 J/g･°C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)

A 0.554 g sample of steam at 106.0 °C is condensed into a container with 5.20 g of water at 16.4 °C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18, the specific heat of steam is 2.01 g., and AH vap = 40.7 kJ/mol. T₁ = °C

What amount of heat , in kj, is required to vaporized 190.55 g of ethanol (C2H5OH)?(Hvsp=43.3 KJ/mol)

When 95.0 grams of ethanol condenses to liquid, how much energy is lost? H(vap) 38.6 kJ/mol and H(fus) 4.60 kJ/mol are the heats of vaporization and fusion, respectively, for ethanol. Ethanol has a molecular weight of 46.

What quantity of heat, in kJ, is required to convert 12.0 g of ethanol (C₂H₂OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g C; AHvap = 39.3 kJ/mol) ●

Table B Physical Constants for Water 334 /g Heat of Fusion 2260 J/g Heat of Vaporization 4.18 J/g•K Specific Heat Capacity of H,O(e)

Enter your answer in the provided box. From the data below, calculate the total heat (in J) needed to convert 0.821 mol of gaseous ethanol at 300.0°C and 1 atm to liquid ethanol at 25.0°C and 1 atm: b.p. at 1 atm: 78.5°C Cgas: 1.43 J/g °C AHⓇ : 40.5 kJ/mol vap Cliquid 2.45 J/g.°C