What amount of heat (in kJ) is required to convert 18.3 g of an unknown liquid (MM = 67.44 g/mol) at 43.5 °C to a gas at 128.2 °C? (specific heat capacity of liquid = 1.18 J/g･°C; specific heat capacity of gas = 0.792 J/g･°C; ∆Hvap = 30.1 kJ/mol; Tb = 97.4°C)

How much energy is required to vaporize 178 g of butane (C 4H 10) at its boiling point, if its ΔH vap is 24.3 kJ/mol?

What amount of heat is required to convert 10.9 g of an unknown liquid (MM 83.21 g/mol) at 19.2°C to a gas at 93.5 °C? (heat capacity of iquid 1.58 J/g.C; heat capacity of gas 0.932 JIg.°C; AHvap 22.5kJ/mol, Tb= 57.3°C) kJ

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 459.3 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C. (heat capacity of solid = 2.96 J/g･°C; heat capacity of liquid = 1.75 J/g･°C; ∆Hfus = 8.04 kJ/mol; normal freezing point, Tf = 17.6 °C) How much energy (in kJ) is absorbed/released to heat the solid?

A 124.0 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 \deg C to 147.6 \deg C. ( heat capacity of liquid = 1.62 J/g. \deg C; heat capacity of gas = 1.04 J/g. \deg C; AHvap = 78.11 kJ/mol; normal boiling point, Tb = 160.3 \deg C) How much energy (in kJ) is absorbed/released to condense the gas?

How much heat (q) in joules (J) was involved when 52.4 g of steam was condensed  (DHvapH2O = 2260 J/g) with a phase change at the boiling point of water?

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/mol

A 0.580 g0.580 g sample of steam at 107.3 ∘C107.3⁢ ∘C is condensed into a container with 4.56 g4.56 g of water at 17.0 ∘C.17.0⁢ ∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18  J g⋅ ∘C,4.18  J g⋅ ∘C, the specific heat of steam is 2.01  J g⋅ ∘C,2.01  J g⋅ ∘C, and Δ?vap=40.7 kJ/mol.

Determine the amount of heat (in kJ) required to convert 8.24 moles of liquid methanol at-22°C into gaseous methanol at 98°C. Use the following information on methanol to calculate the amount of heat for each of the steps. Melting Point =-98°C Boiling Point = 65°C Molar Heat Capacities: Ciquid = 81.1 J/mol °C Cgas = 43.9 J/mol °C AHucion 3.22 kJ/mol AHvaporization 37.3 kJ/mol Type your numeric answer and submit