Answer : The value of [tex]\Delta H[/tex] for the reaction is, -565.6 kJ
Explanation :
First we have to calculate the molar mass of CO.
Molar mass CO = Atomic mass of C + Atomic mass of O = 12 + 16 = 28 g/mole
Now we have to calculate the moles of CO.
[tex]\text{Moles of }CO=\frac{\text{Mass of }CO}{\text{Molar mass of }CO}=\frac{1g}{28g/mole}=\frac{1}{28}mole[/tex]
Now we have to calculate the value of [tex]\Delta H[/tex] for the reaction.
The balanced equation will be,
[tex]2CO(g)+O_2(g)\rightarrow 2CO_2(g)[/tex]
From the balanced chemical reaction we conclude that,
As, [tex]\frac{1}{28}mole[/tex] of CO release heat = 10.1 kJ
So, 2 mole of CO release heat = [tex]2\times 28\times 10.1=565.6kJ[/tex]
Therefore, the value of [tex]\Delta H[/tex] for the reaction is, -565.6 kJ (The negative sign indicates the amount of energy is released)
