A) Hydrazine (NH2NH2), hydrogen peroxide (H2O2), and water all have surface tensions much higher than other substances of comparable molecular weight. The type of intermolecular forces acting in all these three compounds that are responsible for their high surface tension is: (a) ionic bonding (b) hydrogen bonding (c) dispersion forces (d) covalent bonding B) Which phase transition is an endothermic process? (a) Freezing (b) Melting (c) Deposition (d) Condensation C) If ΔH = -54.74 kJ for a chemical rxn, that rxn is: (a) in equilibrim (b) exothermic (c) endothermic (d) may not go to completion D) Calculate the enthalpy change for combustion of methane ∆H°c if the following enthalpies of formation ∆H°f are given: CH4(g) -74.60 kJ/mol H2O(l) -285.8 kJ/mol CO2(g) -393.5 kJ/mol (a) -890.5 kJ/mol (b) 890.5 kJ/mol (c) -1.04x103 kJ/mol (d) 1.04x10-3 kJ/mol
A) Hydrazine (NH2NH2), hydrogen peroxide (H2O2), and water all have surface tensions much higher than other substances of comparable molecular weight. The type of intermolecular forces acting in all these three compounds that are responsible for their high surface tension is:
(a) ionic bonding (b) hydrogen bonding (c) dispersion forces (d) covalent bonding
B) Which phase transition is an endothermic process?
(a) Freezing (b) Melting
(c) Deposition (d) Condensation
C) If ΔH = -54.74 kJ for a chemical rxn, that rxn is:
(a) in equilibrim (b) exothermic
(c) endothermic (d) may not go to completion
D) Calculate the enthalpy change for combustion of methane ∆H°c if the following enthalpies of formation ∆H°f are given: CH4(g) -74.60 kJ/mol
H2O(l) -285.8 kJ/mol
CO2(g) -393.5 kJ/mol
(a) -890.5 kJ/mol (b) 890.5 kJ/mol (c) -1.04x103 kJ/mol (d) 1.04x10-3 kJ/mol
(e) None of those. If som what is your answer?
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