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SiBr_4(l) + 2 H_2O(l) --> SiO_2(s) + 4Hbr(g) formulate a separate, balanced equation for each reactant or product compound showing its formation from...

SiBr_4(l) + 2 H_2O(l) --> SiO_2(s) + 4Hbr(g)


formulate a separate, balanced equation for each reactant or product compound showing its formation from elements in their standard forms and its given ΔH⁰f .


Remember that formation equations show the formation of 1 mole of the compound of interest from elements in their most stable states (at standard ambient temperature and pressure) and must be balanced. (Use the lowest possible coefficients. In order to maintain the correct stoichiometry, this may include fractional coefficients. Include states-of-matter under the given conditions in your answer.)

SiBr4(l):



 


 ΔH⁰f  SiBr4(l) = ______ kJ/mol


H2O(l):



ΔHf ° H2O(l) =  ______kJ/mol


SiO2(s)

 

ΔH⁰f  SiO2(s) =  ______kJ/mol


HBr(g):

 


 

ΔH⁰f  HBr(g) =  _____kJ/mol




Write a balanced chemical equation using the smallest integer coefficients that correctly represent the stoichiometric ratios in the balanced reaction.

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