MCQ
$\Delta {H^o}$ combustion of $C_4H_{10}(g)$ is $-2650\, kJ\, mol^{-1}$ the amount of heat evolve at constant pressure that can be obtained by burning $5.8\, kg$ of $C_4H_{10}$ is approx
  • A
    $2.65 \times {10^3}\,kJ$
  • B
    $265 \times {10^5}\,kJ$
  • $2.65 \times {10^5}\,kJ$
  • D
    $2.65 \times {10^4}\,kJ$

Answer

Correct option: C.
$2.65 \times {10^5}\,kJ$
c
moles of $\mathrm{C}_{4} \mathrm{H}_{10}=\frac{5.8 \times 1000}{58}=100$

Heat evolve due to $100$ moles of $\mathrm{C}_{4} \mathrm{H}_{10}$

$=2650 \times 100$

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