2BrF3(g)Br2(g) + 3F2(g) STANDARD ENTHALPY?
With no arrows I don't know where the reactants end and products start; however,
dHrxn = (n*dHf products) - (n*dHf reactants)
dHformation numbers can be found in your text/notes/web.
To determine the standard enthalpy change for the reaction:
2BrF3(g) → Br2(g) + 3F2(g)
You would need to find the standard enthalpy of formation for each compound involved in the reaction, and then use these values to calculate the enthalpy change.
The standard enthalpy of formation (ΔHf°) is the enthalpy change when 1 mole of a compound is formed from its constituent elements in their standard states (i.e., at 1 atmosphere pressure and a specified temperature, usually 25°C).
Here are the standard enthalpy of formation values you would need for this calculation:
ΔHf°(BrF3) = -238.1 kJ/mol (source: NIST Chemistry WebBook)
ΔHf°(Br2) = 31.9 kJ/mol (source: NIST Chemistry WebBook)
ΔHf°(F2) = 0 kJ/mol (by convention, the standard enthalpy of formation for an element in its standard state is always defined as 0 kJ/mol)
The enthalpy change for the reaction can be calculated using the formula:
ΔH° = ∑(nΔHf°products) - ∑(nΔHf°reactants)
Let's substitute the values:
ΔH° = (2 × ΔHf°(Br2)) + (3 × ΔHf°(F2)) - (2 × ΔHf°(BrF3))
= (2 × 31.9 kJ/mol) + (3 × 0 kJ/mol) - (2 × -238.1 kJ/mol)
= 63.8 kJ/mol + 0 kJ/mol + 476.2 kJ/mol
= 540 kJ/mol
Therefore, the standard enthalpy change for the reaction 2BrF3(g) → Br2(g) + 3F2(g) is 540 kJ/mol.
To determine the standard enthalpy change for the reaction 2BrF3(g) → Br2(g) + 3F2(g), we need to consult a reliable source that provides the standard enthalpy of formation values for each compound involved.
The standard enthalpy of formation (ΔHf) is the change in enthalpy when one mole of a compound is formed from its constituent elements, with each component in its standard state.
Using the known values of the standard enthalpy of formation, we can calculate the standard enthalpy change for the given reaction using the following equation:
ΔH° = Σ(n * ΔHf° products) - Σ(m * ΔHf° reactants)
Where ΔH° is the standard enthalpy change, n and m are the stoichiometric coefficients of the products and reactants, and ΔHf° is the standard enthalpy of formation.
Unfortunately, without access to a reliable source of standard enthalpy of formation data, I cannot provide you with an exact numerical value for the standard enthalpy change of the given reaction. However, you can look up these values in a chemistry reference book or online database to calculate the standard enthalpy change.