The enthalpy of combustion of C, H , and...

The enthalpy of combustion of C, H , and sucrose are -393.5 , -286.2, and -5644.2 kJ/mol calculate the enthalpy of formation of sucrose .

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The enthalpies of combustion of carbon and carbon monoxide are -393.5 and -283 kJ mol^(-1) respectively. The enthaly of formation of carbon monoxide per mole is :

The enthalpies of combustion of diamond and graphite are - 395.4 kJ and - 393.5 kJ respectively calculate the enthalpy of transformation from diamond to graphite.

The heat of combustion of C, S and CS_(2) are -393.3kJ, -293.7kJ and -1108.76kJ. What will be the heat of formation of CS_(2) ?

Standard enthalpy of combustion of cyclopropane is -2091 kJ//"mole" at 25^(@)C then calculated the enthalpy formation of cyclopropane. If DeltaH_(f)^(o)(CO_(2))= -393.5 kJ//"mole" and Delta H_(f)^(o)(H_(2)O)= -285.8 kJ//"mole" .

The heats of combustion of carbon,hydrogen and acetylene are -394kJ, -286kJ and -1301kJ respectively. Calculate heat of formation of C_(2)H_(2)

Ethylene on combustion gives carbon dioxide and water. Its heat of combustion is 1410.0 kJ mol^(-1) . If the heat of formation of CO_(2) and H_(2)O are 393.3 kJ and 286.2 kJ , respectively. Calculate the heat of formation of ethylene.

The enthalpy of formation of H_(2)O(l) is -280.70 kJ/mol and enthalpy of neutralisation of a strong acid and strong base is -56.70 kJ/mol. What is the enthalpy of formation of OH^(-) ions?

The enthalpies of formation of CO2(g),H2O(l) and C2H4(g) are respectively −393.5,−286 and +52.3kJmol −1 . The enthalpy change for the combustion of C2H4(g) is ?

If the enthalpy of combustion of diamond and graphite are -395.4 kJ mol^(-1) and -393.6 kJ mol^(-1) , what is enthalpy change for the C("graphite") rarr C("diamond") ?

ICSE-SELF ASSESSMENT PAPER 03-Questions

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