When the reddish brown mercury (II) oxide, HgO, is heated, it decomposes to its

ID: 840289 • Letter: W

Question

When the reddish brown mercury (II) oxide, HgO, is heated, it decomposes to its elements, liquid mercury and oxygen gas:

HgO(s) ? Hg (l) + O2 (g)

15. If 2.00g of mercury (II) oxide is decomposed, what is the mass of mercury liquid produced?

When lead(II) nitrate is added to an aqueous solution of sodium iodide, a precipitation reaction occurs that removes the iodide ion from solution.

Pb(NO3)2 (aq) + NaI (aq) ? PbI2 (s) + NaNO3 (aq)

16. If a solution contains 7.00g of NaI, what mass of lead(II) nitrate should be added to remove all of the iodide ion from solution?

When the reddish brown mercury (II) oxide, HgO, is heated, it decomposes to its elements, liquid mercury and oxygen gas:

2HgO(s) --->2Hg (l) + O2 (g)

15. If 2.00g of mercury (II) oxide is decomposed, what is the mass of mercury liquid produced?

2(216.6g/mole)--->2(200.6g/mole) +32g/mole (divide whole eq by 216.6)

2g(HgO)----->1.85g(Hg) + 0.148g(O2)

hence liquid Hg produced=1.85g

When lead(II) nitrate is added to an aqueous solution of sodium iodide, a precipitation reaction occurs that removes the iodide ion from solution.

Pb(NO3)2 (aq) + 2NaI (aq) ---->PbI2 (s) + 2NaNO3 (aq)

16. If a solution contains 7.00g of NaI, what mass of lead(II) nitrate should be added to remove all of the iodide ion from solution?

331.2g/mole + 2(149.9g/mole)----->461g/mole + 2(85g/mole)

(since NaI is only 7g so divide whole equation by 42.83

7.73g(Pb(NO3)2) + 7g(NaI)------->10.76g(PbI2) + 3.97g(NaNO3)

hence mass of Pb(ii)nitrate is 7.73g

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