Part A Which gas will remain in the system after the reaction is complete? NH3 o

Question

Part A

Which gas will remain in the system after the reaction is complete?

NH3

or

HCl

Part B

What will be the final pressure of the system after the reaction is complete? (Neglect the volume of the ammonium chloride formed.)

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Part C

What mass of ammonium chloride will be formed?

Pfinal =   atm   Constants | Periodic Table Ammonia, NH3 (g), and hydrogen chloride, HC1(g) react to form solid ammonium chloride, NH4Cl(s) NH3 (g) + HCl(g) ? NH, Cl (s) wo 1.50 L flasks at 30.0C are connected by a topcock, as shown in the drawing NH3(8) HCI(g) One flask contains 6.00gNH3 (g), and the other contains 4.60 g HCl(g). When the stopcock is opened, the gases react until one is completely consumed

Explanation / Answer

Moles of NH3 = mass/molecular weight

= 6g / 17g/mol

= 0.3529 mol

Moles of HCl = mass/molecular weight

= 4.60g / 36.5g/mol

= 0.126 mol

From the stoichiometry of the reaction

Moles of NH3 consumed = moles of HCl consumed

= 0.126 mol

Limiting reactant = HCl

Excess reactant = NH3

Part A

NH3 gas will remain in the system after the reaction is complete

Part b

Moles of NH3 remain = 0.3529 - 0.126 = 0.2269 mol

Final pressure based on the NH3

= nRT/V

= 0.2269 mol x 0.0821 L-atm/mol-K x (30+273)K / (2*1.5L)

= 1.88 atm

Part C

Moles of ammonium chloride will be formed

= moles of HCl consumed

= 0.126 mol

Mass of ammonium chloride will be formed

= moles x molecular weight

= 0.126 mol x 53.491 g/mol

= 6.74 g

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