Answer : The value of
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.
![\text{Moles of }CO=\frac{\text{Mass of }CO}{\text{Molar mass of }CO}=\frac{1g}{28g/mole}=\frac{1}{28}mole](https://tex.z-dn.net/?f=%5Ctext%7BMoles%20of%20%7DCO%3D%5Cfrac%7B%5Ctext%7BMass%20of%20%7DCO%7D%7B%5Ctext%7BMolar%20mass%20of%20%7DCO%7D%3D%5Cfrac%7B1g%7D%7B28g%2Fmole%7D%3D%5Cfrac%7B1%7D%7B28%7Dmole)
Now we have to calculate the value of
for the reaction.
The balanced equation will be,
![2CO(g)+O_2(g)\rightarrow 2CO_2(g)](https://tex.z-dn.net/?f=2CO%28g%29%2BO_2%28g%29%5Crightarrow%202CO_2%28g%29)
From the balanced chemical reaction we conclude that,
As,
of CO release heat = 10.1 kJ
So, 2 mole of CO release heat = ![2\times 28\times 10.1=565.6kJ](https://tex.z-dn.net/?f=2%5Ctimes%2028%5Ctimes%2010.1%3D565.6kJ)
Therefore, the value of
for the reaction is, -565.6 kJ (The negative sign indicates the amount of energy is released)