91Ó°ÊÓ

Here, we must determine what amount of carbon monoxide must be burned in order to emit 175 kJ of heat.

The reaction of combustion of carbon monoxide is shown below

\[{\bf{CO(g) + }}\frac{{\bf{1}}}{{\bf{2}}}{{\bf{O}}_{\bf{2}}}{\bf{(g) }} \to {\bf{ C}}{{\bf{O}}_{\bf{2}}}{\bf{(g) , \Delta H}}_{\bf{c}}^{\bf{^\circ }}{\bf{ = - 283}}{\bf{.0 kJmo}}{{\bf{l}}^{{\bf{ - 1}}}}\]

From the above stoichiometric balanced equation, we can observe that for combustion of 1 mole of carbon monoxide, \[\frac{1}{2}\]mole of oxygen is needed, and the amount of energy released is 283.0 kJ.

We need to follow the steps to find out the no of moles of carbon monoxide required.

\(\begin{aligned}{\rm{ 283kJ heat is produce when 1 mole of carbon monoxide is burnt}}\\{\rm{175kJ heat will be produced when }}\frac{{{\rm{1 mole \times 175 kJ}}}}{{{\rm{283 kJ}}}}{\rm{of carbon monoxide is burnt}}\\{\rm{ = 0}}{\rm{.6183 mol of carbon monoxide }}\end{aligned}\)

To find out the amount of mass of carbon monoxide, follow the steps below.

\[\begin{aligned}{\rm{ Molecular\;mass\;of\;1 \;mole\; of\; carbon \;monoxide\; is \;28 g}}{\rm{.}}\\{\rm{Weight \;of \;0}}{\rm{.6183\; mole \;of\; carbon \;monoxide\; is\; (0}}{\rm{.6183 \times 28)g}}\\{\rm{ = 17}}{\rm{.3124 g}}\end{aligned}\]

Hence, 17.3124 g of carbon monoxide must be burned to produce 175 kJ of heat under standard conditions.