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

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

Use the following reactions to help solve for the net value:

1) SnCl2(s) + TiBr2(s) -> SnBr2(s) + Ticl2(s) Delta H=+4.2

2) SnCl2(s) + Cl2(g) -> TiCl4(l) deltaH=-195

3) TiCl2(s) + Cl2(g) ->TiCl4(l) deltaH=-273

SnCl2(s) + Cl2(g) -> SnCl4(l) deltaH=-195

TiCl4(l) -> TiCl2(s) + Cl2(g) deltaH=+273

SnCl2(s) + TiCl4(l) -> TiCl2(s) + SnCl4(l) deltaH net = +78kJ

Everything that I have posted is exactly what was stated in the problem so I guess everything is in kJ.

To find the value of ΔHnet for the given equation, we need to use Hess's law, which states that the enthalpy change of a reaction is independent of the pathway taken between the initial and final states.

We can start by adding the given reactions together in a way that cancels out the common compounds.

1) SnCl2(s) + TiBr2(s) -> SnBr2(s) + TiCl2(s) (ΔH=+4.2 kJ)
2) SnCl2(s) + Cl2(g) -> TiCl4(l) (ΔH=-195 kJ)
3) TiCl2(s) + Cl2(g) ->TiCl4(l) (ΔH=-273 kJ)
4) SnCl2(s) + TiCl4(l) -> TiBr2(s) + SnCl4(l) (ΔHnet = ?)

Now, we need to manipulate the given reactions so that they match the overall reaction we want to solve for. Let's use stoichiometry to reach the desired compound coefficients.

To match the TiBr2 in the net equation, we multiply reaction (1) by 1, reaction (2) by 2, and reaction (3) by 1.
1) SnCl2(s) + TiBr2(s) -> SnBr2(s) + TiCl2(s) (ΔH=+4.2 kJ)
2) 2SnCl2(s) + Cl2(g) -> 2TiCl4(l) (ΔH=-390 kJ)
3) TiCl2(s) + Cl2(g) ->TiCl4(l) (ΔH=-273 kJ)
4) SnCl2(s) + TiCl4(l) -> TiBr2(s) + SnCl4(l) (ΔHnet = ?)

Now we sum up reactions (2) + (3) to cancel out the TiCl4 compound.

2) 2SnCl2(s) + Cl2(g) -> 2TiCl4(l) (ΔH=-390 kJ)
3) TiCl2(s) + Cl2(g) ->TiCl4(l) (ΔH=-273 kJ)
__________
2SnCl2(s) + 2TiCl2(s) + 2Cl2(g) -> 2TiCl4(l) (ΔH = -663 kJ)

Finally, we combine the sum with reaction (1) to obtain the desired reaction with the same compounds on both sides.

2SnCl2(s) + 2TiCl2(s) + 2Cl2(g) -> 2TiCl4(l) (ΔH=-663 kJ)
1) SnCl2(s) + TiBr2(s) -> SnBr2(s) + TiCl2(s) (ΔH=+4.2 kJ)
_____________________
2SnCl2(s) + TiBr2(s) + 2Cl2(g) -> SnBr2(s) + TiCl4(l)

The ΔHnet is calculated by summing up the ΔH values of the reactions involved. Thus:

ΔHnet = ΔHreaction1 + ΔHreaction2

ΔHnet = +4.2 kJ + (-663 kJ)
ΔHnet = -658.8 kJ

Therefore, the value of ΔHnet for the given equation is -658.8 kJ.