Question

Background Info:

The standard enthalpy of formation  (Δ H∘f

)  is the enthalpy change that occurs when exactly 1  mol  of a compound is formed from its constituent elements under standard conditions. The standard conditions are  1  atm  pressure, a temperature of  25  ∘C  , and all the species present at a concentration of  1  M . A "standard enthalpies of formation table" containing  Δ H∘f  values might look something like this: Substance Δ H∘f H (g) 218  kJ/mol H2 (g) 0  kJ/mol Ba(s) 0  kJ/mol B a 2+ (aq) −538.4  kJ/mol C (g) 71  kJ/mol C (s) 0  kJ/mol N (g) 473  kJ/mol O2 (g) 0  kJ/mol O (g) 249  kJ/mol S2 (g) 129  kJ/mol

Question:
What is the balanced chemical equation for the reaction used to calculate  Δ H∘f  of  BaC O3 (s) ? If fractional coefficients are required, enter them as a fraction (i.e. 1/3). Indicate the physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Use ( aq ) for aqueous solution.
EXPRESS ANSWER AS A CHEMICAL EQUATION. Please explain for me too!!!

Answer 1

You will get at first carbon dioxide by burning C:

C+O_2=CO_2

Burn hydrogen to obtain water:

H_2+\frac{1}{2}O_2=H_2O

Combine them:

CO_2+H_2O=H_2CO_3

Now react it with Ba:

Ba+H_2CO_3=BaCO_3+H_2

To sum up, the reaction is Ba+C+\frac{3}{2}O_2=BaCO_3, using hydrogen as a catalyst.

Step-by-step explanation:

Answer 2

You will get at first carbon dioxide by burning C:

`C+O_2=CO_2`
Burn hydrogen to obtain water:

`H_2+(1)/(2)O_2=H_2O`
Combine them:

`CO_2+H_2O=H_2CO_3`
Now react it with Ba:

`Ba+H_2CO_3=BaCO_3+H_2`
To sum up, the reaction is
`Ba+C+(3)/(2)O_2=BaCO_3`, using hydrogen as a catalyst.