Shaalaa.com | enthalpy of bond dissociation, combustion, formation, atomization, sublimation
Calculate C-Cl bond enthalpy from following reaction:
CH3Cl(g) + Cl2(g) → Ch2Cl2(g) + HCl(g) ΔH° = -104KJ
If C-H, Cl-Cl and H-Cl bond enthalpies are 414, 243 and 431 KJ-Mol-1 respectively.
For the reaction: Cl2(g) → 2Cl(g), _______.
(A) ΔH is positive, ΔS is positive
(B) ΔH is positive, ΔS is negative
(C) ΔH is negative, ΔS is negative
(D) ΔH is negative, ΔS is positive
Calculate the work done in the following reaction at 50o C. State whether work is done on the system or by the system.
`"SO"_2("g") + 1/2"O"_(2("g")) rightarrow "SO"_(3("g"))`
Calculate the standard enthalpy of combustion of CH3COOH(l) from the following data:
`Delta_fH^@(CO_2)=-393.3 kJ mol^-1`
`Delta_fH^@(H_2O)=-285.8 kJ mol^-1`
`Delta_fH^@(CH_3COOH)=-483.2 kJ mol^-1`
Calculate ΔH° for the reaction between ethene and water to form ethyl alcohol from the
ΔcH° C2H5OH(l) = -1368 kJ
ΔcH° C2H4(g) = -1410 kJ
Does the calculated ΔH° represent the enthalpy of formation of liquid ethanol?
Calculate the standard enthalpy of the reaction, 2C(graphite) + 3H2(g) → C2H6(g), ΔH° = ?
From the following ΔH° values
a) `C_2H_6(g) + 7/2 O_2(g) -> 2CO_2(g) + 3H_2 O(l)`. ΔH° = -1560kJ
b) `H_2(g) + 1/2 O_2 (g) -> H_2O(l)` ΔH° = -285.8kJ
c) C(graphite) + O2(g) -> CO2(g). ΔH° = -393.5kJ
- Chemical Thermodynamics and Energetic - Free Energy Change for Spontaneous and Non Spontaneous Processes