Find the value of delta H net for the following equation:

SnBr2(s) + TiCl4(l) -> TiBr2(s) + SnCl4(l)

I know that I already posted this once but I am still lost on what to do.

I know that TiCl4=-804.2 and SnCl4=-511.3 but I thought that the values for SnBr2 is 0 as well as for TiBr2.

SnBr2 is not zero.

TiBr2 is not zero.
I don't know what they are but they aren't zero. The only DHf values that are zero are elements which appear in an equation in their normal state. O2(g), H2(g), etc.

How should I go about solving this problem? Am I missing information?

To find the value of delta H net for the given equation, you need to calculate the enthalpy changes for the individual reactions and then add them up.

The enthalpy change for a reaction can be determined using the following equation:

Delta H = sum(n * H(products)) - sum(m * H(reactants))

Where n and m are the stoichiometric coefficients of the products and reactants, respectively, and H is the enthalpy of the substance.

Let's calculate the enthalpy changes for the given equation:

SnBr2(s) + TiCl4(l) -> TiBr2(s) + SnCl4(l)

To determine the enthalpy change for each component, we need the enthalpy values for SnBr2, TiBr2, TiCl4, and SnCl4.

Since you mentioned that the enthalpy values for TiCl4 and SnCl4 are -804.2 and -511.3, respectively, we can use these values in our calculations.

However, you mentioned that the values for SnBr2 and TiBr2 are both zero. If these values are correct, it suggests that SnBr2 and TiBr2 do not undergo any enthalpy changes during this reaction. This is uncommon, as most compounds do have enthalpy changes upon reaction. It may be worth double-checking the values for SnBr2 and TiBr2 or seeking clarification on whether they are indeed zero.

Assuming SnBr2 and TiBr2 have zero enthalpy changes, we can calculate the delta H net as follows:

Delta H net = (1 * H(TiBr2)) + (1 * H(SnCl4)) - (1 * H(TiCl4)) - (1 * H(SnBr2))

Delta H net = (1 * 0) + (1 * -511.3) - (1 * -804.2) - (1 * 0)

Delta H net = 0 + (-511.3) - (-804.2) - 0

Delta H net = 292.9 kJ

Therefore, the value of delta H net for the given equation is 292.9 kJ.