Given the following data:
c(s) + o2(g) + co2(8) ah = -393 kj
2co(g) + o2(g) → 2c02(8) ah = -566 kj
calculate ah for the reaction 2c(s) + o2(g) → co(g).

Explanation:

We have two equations:

(I)   C(s) + O₂(g) ⟶ CO₂(g);     ΔH = -393 kJ

(II) 2CO(g) + O₂(g) → 2C0₂(g); ΔH = -566 kJ  

From these, we must devise the target equation:

(III) 2C(s) + O₂(g) → 2CO(g); ΔH = ?

The target equation has 2C on the left, so you double Equation (I).

When you double an equation, you double its ΔH.

(IV) 2C(s) + 2O₂(g) ⟶ 2CO₂(g); ΔH = -786 kJ

Equation (IV) has 2CO₂ on the right, and that is not in the target equation.

You need an equation with 2CO₂ on the left, so you reverse Equation (II).  

When you reverse an equation, you reverse the sign of its ΔH.  

(V)  2CO₂(g) → 2CO(g) + O₂(g); ΔH = 566 kJ

Now, you add equations (IV) and (V), cancelling species that appear on opposite sides of the reaction arrows.

When you add equations, you add their ΔH values.

You get the target equation (III):

(IV) 2C(s) + 2O₂(g) ⟶ 2CO₂(g);      ΔH = -786 kJ

(V) 2CO₂(g) → 2CO(g) + O₂(g);       ΔH =   566 kJ

(III) 2C(s) +O₂ ⟶ 2CO;                    ΔH = -220 kJ

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.

i don't know people like to fight everywhere rip.