The reaction of 1 Mol of iron metal with 3 Mol aqueous HCI produces 1.5 mol H2 gas, 1 mol aqueous FeCI3, and 87.9 kj of heat. Write a thermochemical equation for this reaction
Sarah, give it a go, I will check your answer.
Fe + 3HCl ==> 1.5 H2 + FeCl3 + 87.9 kJ
it is mostly correct, you have to get the 1.5 to a solid number not a split number
Does anyone know this?
To write a thermochemical equation for this reaction, we need to use the stoichiometric coefficients and the given values of the reaction. Here's how you can do it step-by-step:
Step 1: Write the balanced chemical equation for the reaction:
Fe(s) + 3 HCl(aq) → 1.5 H2(g) + 1 FeCl3(aq)
Step 2: Add the enthalpy change (∆H) to the equation:
Fe(s) + 3 HCl(aq) → 1.5 H2(g) + 1 FeCl3(aq) + 87.9 kJ
Note: The enthalpy change (∆H) is added as a value at the end of the reaction, indicating the heat released or absorbed during the reaction.
Therefore, the thermochemical equation for this reaction is:
Fe(s) + 3 HCl(aq) → 1.5 H2(g) + 1 FeCl3(aq) ∆H = -87.9 kJ
This equation represents the stoichiometric relationship between the reactants and products, as well as the energy change associated with the reaction.