Chemistry, 18.09.2019 04:20 Jasten

Fa solution containing 85.14 g of mercury(ii) nitrate is allowed to react completely with a solution containing 14.334 g of sodium sulfide, how many grams of solid precipitate will be formed? mass: 29.69 g how many grams of the reactant in excess will remain after the reaction? mass: g assuming complete precipitation, how many moles of each ion remain in solution? if an ion is no longer in solution, enter a zero (0) for the number of moles. hg2+ : 0 mol no–3 : 0 mol na+ : 0 mol s2− : 0 mol

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Answer from: graymonky12

The reaction that takes place is:

Hg(NO₃)₂(ac) + Na₂S(ac) → HgS(s) + 2Na⁺ + 2NO₃⁻

Now we calculate the moles of each reagent -using the molecular weights-, in order to determine the limiting reactant:

Moles of mercury (II) nitrate = 85.14 g * $\frac{1mol}{324.7g}$ =0.2622 moles.Moles of sodium sulfide = 14.334 g * $\frac{1mol}{78.04g}$ =0.1837 moles.

Because the stoichiometric ratio between the reactants is 1:1, we compare the number of moles of each one upfront.

moles Hg(NO₃)₂ > moles Na₂S

Thus Na₂S is the limiting reagent.

So in order to find the mass of solid precipitate, we must calculate it using the moles of Na₂S:

$0.1837 molNa_{2} S*\frac{1molHgS }{1molNa_{2}S}*\frac{232.66g}{1molHgS} =42.740g$

The mass of the solid precipitate is 42.760 g.

In order to calculate the grams of the reactant in excess that will remain after the reaction, we convert the moles that reacted into mass and substract them from the original mass:

Mass of Hg(NO₃)₂ remaining = $85.14g-(0.1837molHg(NO_{3})_{2} * 324.7 g/mol)=25.49g$

The mass of the remaning reactant in excess is 25.49 g.

Because we assume complete precipitation, there are no more Hg⁺² or S⁻² ions in solution. The moles of NO₃⁻ and Na⁺ in solution remain the same during the reaction, so the number is calculated from the number added in the reactant:

Hg⁺²: 0 mol

NO₃⁻: $0.2622molHg(NO_{3})_{2} *\frac{2molNO_{3}^{-}}{1molHg(NO_{3})_{2} *} =0.5244molNO_{3}^{-}$

Na⁺: $0.1837molNa_{2} S*\frac{1molNa^{+}}{1molNa_{2}}=0.1837molNa^{+}$

S²⁻: 0 mol

Answer from: Quest

a mercury barometer is a device that uses the physical properties of mercury in a tube to measure barometric pressure. mercury barometers are used for : -

1. measurement of atmospheric pressure

2. determining the altitude of a place

3. weather forecasting

4. calibration and checking of aneroid barometers

5. application in fluid mechanics

6. measurement of pressure in aircrafts

7. surface weather analysis

8. preparation of barographs

9. usage in physical sciences like physics, astronomy & chemistry

10. preparation of aircraft altimeters

characteristics of mercury barometer : -

1.used to define and measure atmospheric pressure.

2.on the average at sea level the column of mercury rises to a height of about 760 mm.

3.this quantity is equal to 1 atmosphere.

4.it is also known as standard atmospheric pressure.

5.a barometer in which the weight of a column of mercury in a glass tube with a sealed top is balanced against that of the atmosphere pressing on an exposed cistern of mercury at the base of the mercury column, the height of the column varying with atmospheric pressure.

Write 15 uses of a mercury barometer along with its characterestics

Answer from: Quest

the answer is barium and copper bromide

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