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tealweasel435Lv1

11 Dec 2019

For a reaction to be endothermic, which of the following relationships is valid?

The energy required to break bonds is greater than the energy involved in bond formation.

The energy required to break bonds is less than the energy involved in bond formation.

The energy required to break bonds is the same as the energy involved in bond formation.

The number of bonds broken equals the number of bonds formed.

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1 Dec 2020

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In the following reactionCH4+CH4 arrow CH3CH3+H2two C-H bonds are broken(bond energy =412 kj/mol) to form a new C-C bond(bond energy=348 kj/mol and a new H-H bond(bond energy=436 kj/mol). Estimate the enthalpy in this reaction. Is it endothermic or exothermic:Hint for exothermic reactions the combined energies of the new bonds should be larger than the combined energies of the broken bonds.Balanced the following unbalanced reaction and calculate its standard free energy change(under standard reactions). State whether the reaction is spontaneous or nonspontaneous under standard conditionsC2H5OH(l)+O2(g) arrow CO2(g)+H2O(l) C2H5OH(l) O2(g) CO2(g) H2O(l) deltaH kj/mol -277.7 0 -393.5 -285.8 deltaG kjmol -174.8 0 -394.4 -237.1

Just answer

Which statement(s) is/are true about bond enthalpy?

a) The bond energy for a triple bond between A and B is three times that of a single bond between A and B

b) for breaking of a bond is always a negative number

c) Energy is required to make a bond

d) Bond enthalpy is defined only for the bonds broken or formed in the gaseous state

e) The presence of bonds does not influence the geometry of the molecule. However, the presence of bonds affects the value of the bond enthalpy between two atoms

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	The energy required to break bonds is greater than the energy involved in bond formation.
	The energy required to break bonds is less than the energy involved in bond formation.
	The energy required to break bonds is the same as the energy involved in bond formation.
	The number of bonds broken equals the number of bonds formed.