1. Tardigrade
  2. Question
  3. Chemistry
  4. 28.0 L of CO 2 is produced on complete combustion of 16.8 L gaseous mixture of ethene and methane at 25° C and 1 atm. Heat evolved during the combustion process is kJ. Given: Δ H c ( CH 4)=-900 kJ mol -1 Δ H c ( C 2 H 4)=-1400 kJ mol -1

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. $28.0\, L$ of $CO _2$ is produced on complete combustion of $16.8 \, L$ gaseous mixture of ethene and methane at $25^{\circ} C$ and $1 \, atm$. Heat evolved during the combustion process is ______$kJ$.
Given : $\Delta H _{ c }\left( CH _4\right)=-900 \, kJ\, mol ^{-1}$
$\Delta H _{ c }\left( C _2 H _4\right)=-1400\, kJ \, mol ^{-1}$

JEE MainJEE Main 2023Thermodynamics

Solution:

image
$\Rightarrow 28=16.8+ x $
$x =11.2 L $
$ n _{ CH _4}=\frac{ PV }{ RT }=\frac{1 \times 5.6}{0.082 \times 298}=0.229 \text { mole }$
$ n _{ C _2 H _2}= \frac{11.2}{0.082 \times 298}=0.458 \text { mole } $
$\therefore \text { Heat evolved }=0.229 \times 900+0.458 \times 1400 $
$=206.1+641.2 $
$= 847.3 \,kJ$