1) Determine the value of delta H net for the following equation:
SnBr2(s) + TiCl4(l) -> TiBr2(s) + SnCl4(l)
I am not sure how to solve this.
delta Hf = dHf
dHrxn = (n*dHf products) - (n*dHf reactants)
for TiCl4 i got -804.2 and for SnCl4 I got -511.3 and then i subtracted them to get -292.9 but I don't think this is right.
You didn't use ALL of the products nor ALL of the reactants.
To determine the value of ΔH net for the given equation, you need to consider the enthalpies of formation for each compound involved in the reaction. The ΔH net can be calculated using the equation:
ΔH net = ΣnΔHf(products) - ΣnΔHf(reactants)
Where:
ΔH net is the net enthalpy change
n is the stoichiometric coefficient of each compound
ΔHf(products) is the enthalpy of formation for each product compound
ΔHf(reactants) is the enthalpy of formation for each reactant compound
First, you'll need to find the enthalpies of formation (ΔHf) for each compound involved in the reaction. These values can usually be found in a table of thermodynamic data.
After obtaining the ΔHf values for the reactants and products (SnBr2, TiCl4, TiBr2, and SnCl4), you can substitute these values into the equation and calculate ΔH net. Remember to take into account the stoichiometric coefficients of each compound.
Lastly, ensure that the ΔHf values are given in the same units as the stoichiometric coefficients. If not, you may need to adjust the values accordingly.
By following these steps, you should be able to calculate the value of ΔH net for the given equation.