JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry
For complete combustion of ethanol, \(C_2H_5OH_{(l)}+{3O_2} _{(g)} \rightarrow 2{CO_2} _{(g)}+3{H_2O}_{(l)}\) the amount of heat produced as measured in bomb calorimeter, is \(1364.47\, kJ\, mol^{-1}\) at \(25\,^oC.\) Assuming ideality the enthalpy of combustion, \(\Delta_CH,\) for the reaction will be : \((R = 8.314\,kJ \,mol^{-1})\) .....\(kJ\, mol^{-1}\)
- A \(- 1366. 95\)
- B \(- 1361.95\)
- C \(- 1460.95\)
- D \(- 1350. 50\)
Answer & Solution
Correct Answer
(A) \(- 1366. 95\)
Step-by-step Solution
Detailed explanation
\(C _{2} H _{5} OH ( l )+3 O _{2}( g ) \rightarrow 2 CO _{2}( g )+3 H _{2} O ( l )\) \(\Delta E =-1364.47 kJ mol ^{-1}\) \(\Delta H =?\) \(T =298 K\) \(\Delta n _{ g }=-1 \because\) complete combution \(R =8.314 J mol ^{-1}=\frac{8.314}{1000} kJ mol ^{-1}\)…
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