What is the Diference between integral enthalpy of solution and differential enthalpy of solution (at least 3 points)

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Integral enthalpies of solution - the enthalpy change in the process of dissolution of a finite number of mol of the substance in the final number of mole of solvent. And differential enthalpies of solution - referred to 1 mol of a substance the enthalpy change upon dissolution of the infinite small number of mol of to the final amount of solvent or the enthalpy change upon dissolution of a finite number of mol of the substance in an infinitely large quantity of solvent.

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Integral enthalpies of solution - the enthalpy change in the process of dissolution of a finite number of mol of the substance in the final number of mole of solvent. And differential enthalpies of solution - referred to 1 mol of a substance the enthalpy change upon dissolution of the infinite small number of mol of to the final amount of solvent or the enthalpy change upon dissolution of a finite number of mol of the substance in an infinitely large quantity of solvent.

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the molar enthalpy of combustion of ethanol (c2H5OH) is -1366.8kj/mol what is the enthalpy change when 10.00 grams of ethanol is combusted

n(C2H5OH)=m/M=10/46 = 0.2174 molH= (-1366.8)*0.2174 = -297.14 kJAnswer: -297.14 kJ

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How many grams of water can be frozen at 0 <sup>o </sup>C with the removal of -129.8 J? (Specific Heat = 4.2 𝐽/𝑔<sup>o</sup>𝐶, Enthalpy of fusion 6010 J/mol, Enthalpy of vaporization = 40700 J/mol)

Number of moles frogen = 6010 / 129.8 = 46.3 mol .Mass of H2O = ( 46.3 × 18 ) g = 832 . 1538

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The standard enthalpy of the reaction: CO(NH2)24) + H20) -› CO2(g) + 2 NHa(a) is -133.42 kJ/mol. Calculate the standard enthalpy of formation of urea, CO(NH2)2(6).

Standard enthalpy of formation=-362kJ/mol

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the standard enthalpy of formation of urea, CO(NH2)2(6). The standard enthalpy of the reaction: CO(NH2)2() + H2Om) -› COz) + 2 NHare) is -133.42 kJ/mol. Calculate

Standard enthalpy of formation=-362kJ/mol

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which group has highest atomic radius , ionisation enthalpy, electron gain enthalpy , electronegativity.

Highest atomic radius has Francium. The nobel gases have the highest ionisation enthalpy. Halogens have high value of electron gain enthalpy. Florine has highest electronegativity.

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Explain the following terms: i) Integral enthalpy of solution ii) Differential enthalpy of solution iii) Enthalpy of dilution

I. Integral Enthalpy Of Solution is the heat absorbed or released when a solute is dissolved in a definite amount of solvent. The heat of solution depends on the nature...

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Justify - H*(CO2) = Delta_f H*(CO2) [*means zero in superscript and _f means f in subscript] where, H* is standard enthalpy and Delta_f H* means standard enthalpy change of formation.

C + O2 --gt; CO2 Delta_f H*(CO2) = H*(CO2) - [H*(C) + H*(O2)] The standard enthalpy of elementary substance is zero: H*(C) = H*(O2) = 0 Therefore Delta_f H*(CO2) =...

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the standard enthalpy of combustion of ethane, carbon, and hydrogen are -1559.7 kJ/mol, -393kJ/mol and -286kJ/mol respectively. Use Hess'ss law to find the enthalpy of formation of ethane

ΔHform(C2H6)=ΔHcomb(C2H6)-(2ΔHcomb(C)+3ΔHcomb(H2))=-1559.7-(2(-393)+3(-286))=84,3 kJ/mol

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Define enthalpy of combustion. Calculate the enthalpy of combustion of methanol if the enthalpies of formation of CO2,H20 andCH3OH are respectively . -393.5kj/mol,-285.8kj/mol and -239.0kj/mol.

Answer: Enthalpy of combustion is the heat released during combustion of one mol amount of any substance by oxygen.You can calculate the combustion enthalpy of methanol using the enthalpy...

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Assuming enthalpy of combustion of hydrogen at 273 K, –286 kJ and enthalpy of fusion of ice at the same temperature to be + 6.0 kJ, calculate enthalpy change during formation of 100 g of ice

Answer: H2 + 1/2O2 = H2O(l) ΔH (H2) =-286 kJ/mol ΔH H2O (s) = H2O(l) =6.0 kJ/mol n = m/M M (H2O) = 18 g/mol n (H2O) = 100 / 18...

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