What amount of heat, in kJ, would be involved in condensing 18.0 g of CH₃OH? (∆Hvap = 38.0 kJ/mol)

Carbon tetrachloride (CCl4) boils at 77∘C. The measured enthalpy of vaporization is 29.8 kJ/mol What is the heat of vaporization?

Calculate the amount of heat needed to raise the temperature of 55.0 g of liquid water from 25°C to 99°C. The specific heat of liquid water is 1.00 cal/g °C

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Calculate the energy (in kcal) required to convert one ice cube that was made by freezing 72 mL of water (density = 1.000 g/L) an an initial temperature of -36.0 C, to liquid water at a final temperature of 37.0 CH2O(s) --> H2O(l) ΔH = +6.02 kj/mol Cpm H2O(s) = 37.7 J/mol x K  Cpm H2O(l) = 75.4 J/mol x K  1 kcal = 4.18 kJ

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Dd.99.

A sample of C3H4Br2 has a normal boiling temperature of 131.5 °C. The enthalpy of vaporization for this compound is 35.4 kJ/mol. How much energy would be required to heat a 13.5 gram sample of liquid C3H4Br2 from 97.5 °C to a gas at 187.2 °C? The specific heat for the liquid is 0.865 J/g °C and the specific heat for the gas is 0.364 J/g. °C.

F103.

How much energy (heat) is required to convert 31.3 g of H2O() at 36.2°C to H2O(g) at 108.6°C? specific heat of ice: 2.09 J/g. C specific heat of water: 4.184 J/g.°C AHfus 6.02 kJ/mol AHvap 40.7 kJ/mol specific heat of steam: 1.84 J/gC Answer = kJ Question 8 Compound A undergoes a reaction with B to proluce C gas and liquid D. The standard heat of combustion of compound A is -1,340.2 kJ/mol. Given that AH (B(g)) - -189.2 kJ/molAH"(C(g)] - 418.4 kJ/mol, AH(C(g)]--418.4 kJ/mol, and AH(D) -258.3 kJ/mol, what is the standard enthalpy of formation of Compound A? A+3 B(g) --> 2 C(g) +3 D) Answer KJ/mol