Background Info: The standard enthalpy of formation (ΔH∘f) is the enthalpy change that occurs when exactly1 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 ΔH∘f values might look something like this:SubstanceΔH∘fH(g)218 kJ/molH2(g)0 kJ/molBa(s)0 kJ/molBa2+(aq)−538.4 kJ/molC(g)71 kJ/molC(s)0 kJ/molN(g)473 kJ/molO2(g)0 kJ/molO(g)249 kJ/molS2(g)129 kJ/mol Question: What is the balanced chemical equation for the reaction used to calculate ΔH∘f of BaCO3(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!!!

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You will get at first carbon dioxide by burning C: [latex]C+O_2=CO_2[/latex] Burn hydrogen to obtain water: [latex]H_2+\frac{1}{2}O_2=H_2O[/latex] Combine them: [latex]CO_2+H_2O=H_2CO_3[/latex] Now react it with Ba: [latex]Ba+H_2CO_3=BaCO_3+H_2[/latex] To sum up, the reaction is [latex]Ba+C+\frac{3}{2}O_2=BaCO_3[/latex], using hydrogen as a catalyst.

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