Calculate δh o rxn for the following: a. sio2(s) + 4 hf(g) → sif4(g) + 2 h2o(l) δh o f [sio2 (s)] = −910.9 kj/mol δh o f [hf (g)] = −273 kj/mol δh o f [sif4 (g)] = −1,614.9 kj/mol δh o f [h2o (l)] = −285.840 kj/mol b. c2h6(g) + o2(g) co2(g) + h2o(g)

Answer : The value of for the reaction is -183.68 kJ/mole

Explanation :

Enthalpy change : It is defined as the difference in enthalpies of all the product and the reactants each multiplied with their respective number of moles. It is represented as

The equation used to calculate enthalpy change is of a reaction is:  

The equilibrium reaction follows:

The equation for the enthalpy change of the above reaction is:

We are given:

Putting values in above equation, we get:

Therefore, the value of for the reaction is -183.68 kJ/mole

i believe it is a.) released into

explanation:

catya your not at all which answer i've seen you do this on another question!