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pedrojulianhdz2005
10.11.2019 •
Chemistry
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)
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Ответ:
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![\Delta H^o](/tpl/images/0367/7523/ae3c5.png)
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
Ответ:
A
More in details:
If the net force acting on an object is zero, its inertia is also zero.