JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry
\(0.3\,g\) of ethane undergoes combustion at \(27^{\circ}\,C\) in a bomb calorimeter. The temperature of calorimeter system (including the water) is found to rise by \(0.5^{\circ}\,C\). The heat evolved during combustion of ethane at constant pressure is \(.......kJ\,mol { }^{-1}\). (Nearest integer) [Given : The heat capacity of the calorimeter system is \(20\, kJ\, K ^{-1}, R =8.3\, JK ^{-1}\, mol ^{-1}\). Assume ideal gas behaviour. Atomic mass of \(C\) and \(H\) are \(12\) and \(1\, g\, mol ^{-1}\) respectively]
- A \(1005\)
- B \(1006\)
- C \(1004\)
- D \(1003\)
Answer & Solution
Correct Answer
(B) \(1006\)
Step-by-step Solution
Detailed explanation
Bomb calorimeter \(\rightarrow\) const volume Heat released By combustion of \(1\) mole \(C _2 H _6(\Delta U )=-\frac{20 \times 0.5}{0.3} \times 30=-1000\,kJ\) \(C _2 H _6( g )+7 / 2 O _2( g ) \rightarrow 2 CO _2( g )+3 H _2 O (l)\) \(\Delta ng =2-(2+7 / 2)=-(7 / 2)\)…
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