Acid –base reactions and gases too! What mass of Na 2 CO 3 ( s ) (in kg) and vol

Question

Acid –base reactions and gases too!

What mass of Na2CO3(s) (in kg) and volume of 2.1 M HNO3 (aq) (in L) are needed to generate 105.8 L of CO2(g) at 291. K and 745. mm Hg pressure by the following (is it balanced) reaction? Note that the reaction proceeds in 95% yield.

HNO3 (aq) + Na2CO3(s) à NaNO3(aq) + H2O (l) + CO2(g)

What is the density of gaseous CO2 under the conditions of temperature and pressure described in part (a) of this question?

Fluorides of sulfur are also gases. Would you expect a balloon filled with CO2 to float or sink in a chamber filled with SF4 when the pressures and temperatures of the SFx and CO2 are the same? Explain your answer clearly, describing and computing at least one important factor.

Extra credit (5 points): correctly name all the compounds in the equation of reaction in part (a).

Explanation / Answer

The reaction is

HNO3 (aq) + Na2CO3(s) à NaNO3(aq) + H2O (l) + CO2(g)

Moles occupies by 105.8L of CO2 at 745 mm Hg and 291K, n= PV/RT

R=0.0821 L.atm/mole.K

P= 745/760 atm=0.98 atm, n= 0.98*105.8/(291*0.0821) =4.33 moles

The reaction proceeds to 95% yield

From the reactino, moles of Na2CO3 = moles of CO2/0.95 =4.57

Molar mass of Na2CO3= 106, mass of Na2CO3= moles * molar mass = 4.57*106 =484 gm

Moles of HNO3= 4.57 ( same as moles of Na2CO3)

Volume of HNO3= moles of HNO3/ its Molarity = 4.57/2.1 L =2.2 L

From gas law. PV= nRT= (mass/molar mass)*RT

P*molar mass = density* RT ( density = mass/ volume)

Density = P* molar mass/ RT = 0.98*44/(0.0821*291)=1.8 g/L

Molar mass of SF4= 104 and molar mass of CO2=44

Density of SF4 under the same conditions = 0.98*104/(0.0821*291)=4.3 g/L

CO2 density is < density of SF4

So CO2 being lighter than SF4, rises in a chamber filled with SF4.

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