Advertisements
Advertisements
प्रश्न
Calculate the enthalpy change for the reaction \[\ce{Fe2O3 + 3CO -> 2Fe + 3CO2}\] from the following data.
\[\ce{2Fe + 3/2O2 -> Fe2O3}\]; ΔH = −741 kJ
\[\ce{C + 1/2O2 -> CO}\]; ΔH = −137 kJ
\[\ce{C + O2-> CO2}\]; ΔH = −394.5 kJ
Advertisements
उत्तर
∆Hf (Fe2O3) = −741 kJ mol−1
∆Hf (CO) = −137 kJ mol−1
∆Hf (CO2) = −394.5 kJ mol−1
\[\ce{Fe2O3 + 3CO -> 2Fe + 3CO2}\]
ΔHr = ?
ΔHr = `Σ (Δ"H"_"f")_"products" − Σ (Δ"H"_"f")_"reactants"`
ΔHr = [2 ∆Hf (Fe) + 3 ∆Hf (CO2)] – [∆Hf (Fe2O3) + 3∆Hf (CO)]
ΔHr = [0 + 3 (−394.5)] − [−741 + 3 (−137)]
ΔHr = [−1183.5] − [−1152]
ΔHr = −1183.5 + 1152
ΔHr = −31.5 kJ mol−1
APPEARS IN
संबंधित प्रश्न
Select the most appropriate option.
Bond enthalpies of H–H, Cl–Cl, and H–Cl bonds are 434 kJ mol–1, 242 kJ mol–1, and 431 kJ mol–1, respectively. Enthalpy of formation of HCl is _______.
Answer in brief.
Obtain the expression for work done in chemical reaction.
Obtain the relationship between ΔH and ΔU for gas phase reactions.
An ideal gas expands from the volume of 1 × 10–3 m3 to 1 × 10–2 m3 at 300 K against a constant pressure at 1 × 105 Nm–2. The work done is
Enthalpy of neutralization is always a constant when a strong acid is neutralized by a strong base: account for the statement.
When 4 g of iron is burnt to ferric oxide at constant pressure, 29.28 kJ of heat is evolved. What is the enthalpy of formation of ferric oxide?
(Atomic mass of Fe = 56)
In which of the following reactions, ΔH is not equal to ΔU?
What is the amount of work done when 0.5 mole of methane, CH4 (g), is subjected to combustion at 300 K? (Given, R = 8.314 JK-1mol-1)
\[\ce{C(s) + 2H2(g) → CH4(g)}\]; ΔH= –74.8 kJ mol−1. Which of the following diagrams gives an accurate representation of the above reaction?
The equilibrium concentrations of the species in the reaction \[ \mathrm{A} + \mathrm{B} \rightleftharpoons \mathrm{C} + \mathrm{D} \] are 2, 3, 10 and 6 mol L-1, respectively at 300 K. ΔGº for the reaction is (R = 2 cal/mol K)
