Write the net ionic and full (molecular) equations for the precipitation reactio

Question

Write the net ionic and full (molecular) equations for the precipitation reaction that occurs when solutions of silver nitrate and potassium carbonate are mixed. Write the equation showing how each of the following ionize or dissociate when dissolved in water, a) HCIO_4, b) HCIO_2, c) KOH Write the molecular and net ionic equations for the reaction that occurs when solutions of HCIO_4 and NaOH are mixed. Given the reaction: 2 ZnS (s) + 3 O_2 (g) rightarrow 2 ZnO (s) + 2 SO_2 (g) Calculate delta H degree for the reaction. (Enthalpies of formation: ZnS (s) (-202.9 W/mol) O_2 (g) (0 kJ/mol). ZnO W (-34S kJ/mol), SO_2 (g) (-296.1 kJ/mol)) Is the reaction exothermic or endothermic? What us delta H degree when 4 32 g of ZnS react? Which have stronger bonds, the reactants or the products?

Explanation / Answer

The balanced conventional equation is: K2CO3(aq) + 2AgNO3(aq) -----------> 2KNO3(aq) + Ag2CO3(s)

Whereas the balanced total ionic equation is:

2K+ (aq) + CO3 2- (aq) + 2Ag+ (aq) + 2NO3 - (aq) ----------> 2K+ (aq) + 2NO3 - (aq) + Ag2CO3(s)

Remove spectator ions (ions that do not change state) 2K+ (aq) and 2NO3 - (aq)

Then the balanced net ionic equation is: CO3 2- (aq) + 2Ag+ (aq) ----------> Ag2CO3(s)

You would observe a precipitate of Ag2CO3 as evidance

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