1. Tardigrade
  2. Question
  3. Chemistry
  4. For the reaction: CO ( g )+(1/2) O 2( g ) arrow CO 2( g ) Δ H°=-67650 cal text at 25° C Calculate Δ H° at 100° C, given that the required molar heat capacities are as follows: CP( CO, gas )=6.97 cal / ° C CP( CO 2., gas )=8.47 cal / ° C CP( O 2., gas )=7.00 cal / ° C

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. For the reaction:
$CO ( g )+\frac{1}{2} O _{2}( g ) \rightarrow CO _{2}( g ) $
$\Delta H^{\circ}=-67650\, cal \text { at } 25^{\circ} C$
Calculate $\Delta H^{\circ}$ at $100^{\circ} C$, given that the required molar heat capacities are as follows:
$C_{P}( CO$, gas $)=6.97 \,cal /{ }^{\circ} C$
$C_{P}\left( CO _{2}\right.$, gas $)=8.47\, cal /{ }^{\circ} C$
$C_{P}\left( O _{2}\right.$, gas $)=7.00\, cal /{ }^{\circ} C$

Thermodynamics

Solution:

$\Delta H_{100}^{\circ}-=\Delta H_{25^{\circ} C }^{\circ}=\left(C_{p_{2}}-C_{p_{2}}\right) \Delta T$
$\Rightarrow \Delta H_{100}^{\circ} =75\left(8.97-6.97-\frac{7}{2}\right)+\Delta H_{25^{\circ} C }^{\circ} $
$=(-112.50-67650) \,cal =-67762.5\, cal $