Advertisements
Advertisements
प्रश्न
The standard enthalpies of formation of SO2 and SO3 are −297 kJ mol−1 and −396 kJ mol−1 respectively. Calculate the standard enthalpy of reaction for the reaction: \[\ce{SO2 + 1/2O2 -> SO3}\]
Advertisements
उत्तर
`Δ"H"_"f"^0` (SO2) = −297 kJ mol−1
`Δ"H"_"f"^0` (SO3) = −396 kJ mol−1
\[\ce{SO2 + 1/2O2 -> SO3}\]
`Δ"H"_"r"^0` = ?
`Δ"H"_"r"^0 = (Δ"H"_"f"^0)_"compound" - sum(Δ"H"_"f")_"elements"`
`Δ"H"_"r"^0 = Δ"H"_"f"^0 ("SO"_3) - [Δ"H"_"f"^0 ("SO"_2) + 1/2 Δ"H"_"f"^0 ("O"_2)]`
`Δ"H"_"r"^0` = −396 kJ mol−1 − (−297 kJ mol−1 + 0)
`Δ"H"_"r"^0` = −396 kJ mol−1 + 297
`Δ"H"_"r"^0` = − 99 kJ mol−1
APPEARS IN
संबंधित प्रश्न
Select the most appropriate option.
If the standard enthalpy of formation of methanol is –238.9 kJ mol–1 then entropy change of the surroundings will be _______.
Write the mathematical relation between ΔH and ΔU during the formation of one mole of CO2 under standard conditions.
The standard enthalpy of formation of ammonia is −46.0 kJ mol−1. The enthalpy change for the reaction:
\[\ce{2NH3_{(g)} -> 2N2_{(g)} + 3H2_{(g)}}\] is ____________.
When 6.0 g of O2 reacts with CIF as per \[\ce{2ClF_{(g)} + O2_{(g)} -> Cl2O_{(g)} + OF2_{(g)}}\] the enthalpy change is 38.55 kJ. The standard enthalpy of the reaction is ____________.
Given the bond energies N ≡ N, H – H and N – H bonds are 945, 436 and 391 kJ/mol respectively. The enthalpy of the reaction;
\[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\]
Work done when 2 moles of an ideal gas is compressed from a volume of 5 m3 to 1 dm3 at 300 K, under a pressure of 100 kPa is ____________.
Calculate ΔU if 2 kJ heat is released and 10 kJ of work is done on the system.
In a particular reaction, 2 kJ of heat is released by the system and 8 kJ of work is done on the system. Determine ΔU.
Define enthalpy.
\[\ce{C(s) + 2H2(g) → CH4(g)}\]; ΔH= –74.8 kJ mol−1. Which of the following diagrams gives an accurate representation of the above reaction?
