Question

Calculate the enthalpy of the reaction 4B(s) + 3O₂ (g) →2B₂O₃ (s) given the following pertinent information 1B₂O₃(s) + 3H₂0(g) - 3O₂(g) 1B₂H₆ (g), 2.2B(s) + 3H₂(g) → B,H-G(g), 3H₂(g)H₂O (g)→ H₂O(1), 4H₂O(l) → H₂O(g), Δ =+2035 kJ Hc = -285 kJ Express your answer with the appropriate units.

Answer 1

To solve the question, we'd use Hess's Law with the correct enthalpy values for the involved reactions, which are not provided in the information given. Once obtained, these values would be combined in a way that leads to the desired reaction, allowing for the calculation of its enthalpy change.

Step-by-step explanation:

To calculate the enthalpy of the reaction 4B(s) + 3O₂ (g) → 2B₂O₃ (s), we need to use Hess's Law which states that the total enthalpy change for a reaction is the same, no matter how many steps it occurs in. Therefore, we must find a way to add up reactions that we know the enthalpy changes for to get the desired reaction for which we want to find the enthalpy change.

Unfortunately, the data provided does not directly help in solving the question as given, because specific enthalpies for the relevant reactions aren't provided. The student will need to obtain the correct enthalpy values for the given reactions (possibly from a standard enthalpy table) and then combine them using Hess's Law to find the desired reaction enthalpy.