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marissa [1.9K]
3 years ago
8

PLEASE LOOK AT POST MARKING BRAINIEST

Chemistry
1 answer:
Charra [1.4K]3 years ago
8 0

Explanation:

             MgF₂ + ___Li₂CO₃  → ___MgCO₃ + ___LiF

1. Every chemical reactions obey the law of conservation of matter. The law states that "matter can neither be created not destroyed but transformed from one form to another".

 When chemical reactions are balanced, they simply obey the law of conservation of matter and mass. This makes makes measurement easy to make when carrying out experiments. One can easily deduce the amount of reactants to be used and the products expeceted

2                 MgF₂ + ___Li₂CO₃  → ___MgCO₃ + ___LiF

  to balance the equation:

  • check if the equation is balanced.
  • Put a,b,c and d before each of the products and reactants.

                  aMgF₂ + bLi₂CO₃  → cMgCO₃ + dLiF

  • The coefficients are needed to balance the equation:

  conserving Mg:       a = c

                       F:         2a = d

                       Li:        2b = d

                        C:        b = c

                        O:       3b = 3c

  • From the above:

       let us assume that    a=1

         then                         c = 1

                                          b = 1

                                          d =2

     

                         MgF₂ + Li₂CO₃  → MgCO₃ + 2LiF

Learn more:

Balanced chemical reaction brainly.com/question/11102790

#learnwithBrainly

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. Determine the standard free energy change, ɔ(G p for the formation of S2−(aq) given that the ɔ(G p for Ag+(aq) and Ag2S(s) are
olga nikolaevna [1]

<u>Answer:</u> The standard free energy change of formation of S^{2-}(aq.) is 92.094 kJ/mol

<u>Explanation:</u>

We are given:

K_{sp}\text{ of }Ag_2S=8\times 10^{-51}

Relation between standard Gibbs free energy and equilibrium constant follows:

\Delta G^o=-RT\ln K

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\Delta G^o = standard Gibbs free energy = ?

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Putting values in above equation, we get:

\Delta G^o=-(8.314J/K.mol)\times 298K\times \ln (8\times 10^{-51})\\\\\Delta G^o=285793.9J/mol=285.794kJ

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The equation used to calculate Gibbs free change is of a reaction is:  

\Delta G^o_{rxn}=\sum [n\times \Delta G^o_f_{(product)}]-\sum [n\times \Delta G^o_f_{(reactant)}]

The equation for the Gibbs free energy change of the above reaction is:

\Delta G^o_{rxn}=[(2\times \Delta G^o_f_{(Ag^+(aq.))})+(1\times \Delta G^o_f_{(S^{2-}(aq.))})]-[(1\times \Delta G^o_f_{(Ag_2S(s))})]

We are given:

\Delta G^o_f_{(Ag_2S(s))}=-39.5kJ/mol\\\Delta G^o_f_{(Ag^+(aq.))}=77.1kJ/mol\\\Delta G^o=285.794kJ

Putting values in above equation, we get:

285.794=[(2\times 77.1)+(1\times \Delta G^o_f_{(S^{2-}(aq.))})]-[(1\times (-39.5))]\\\\\Delta G^o_f_{(S^{2-}(aq.))=92.094J/mol

Hence, the standard free energy change of formation of S^{2-}(aq.) is 92.094 kJ/mol

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Hey there!

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