How much heat is needed to produce 10.5 moles of methane gas
1117.2 kcal
Well, I'm not sure about the exact amount of heat, but you can definitely say it's hotter than a chili pepper eating a jalapeño while sitting in a sauna.
To determine the amount of heat needed to produce 10.5 moles of methane gas, we need to consider the enthalpy change of the reaction involved.
The balanced chemical equation for the combustion of methane (CH4) is:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
The enthalpy change, ΔH, for this reaction is -891 kJ/mol of methane. This means that 891 kJ of heat is released for every mole of methane burned.
To calculate the total amount of heat required to produce 10.5 moles of methane gas, we multiply the number of moles by the enthalpy change:
Total heat required = (10.5 moles) × (-891 kJ/mol)
Calculating this expression will give us the result.
To calculate the amount of heat required to produce a given amount of methane gas, we need to know the enthalpy change associated with the reaction that produces methane. This information is typically provided in a chemical reaction equation along with the stoichiometry of the reactions. In this case, we'll assume we know the balanced chemical reaction equation and the enthalpy change associated with it.
The balanced chemical reaction equation for the production of methane is:
2H₂ + C → CH₄
The enthalpy change (ΔH) for this reaction is -74.6 kJ/mol.
To calculate the amount of heat required to produce 10.5 moles of methane gas, we can use the following equation:
Heat (q) = moles of methane (n) × enthalpy change (ΔH)
Plugging the values into the equation:
q = 10.5 moles × -74.6 kJ/mol
Calculating the result:
q ≈ -781.8 kJ
Therefore, approximately -781.8 kJ of heat is needed to produce 10.5 moles of methane gas. The negative sign indicates that the reaction is exothermic, meaning it releases heat.