For each of the following, which shows the greater deviation ideal behavior at t

Question

For each of the following, which shows the greater deviation ideal behavior at the same set of conditions? Explain. Ammonia and hydrogen chloride react to form solid ammonium chloride: NH_3 (g) + HCl(g) rightarrow NH_4Cl(s) Two 2.00-L flasks at 25 degree C are connected by a valve, as shown in the drawing on the next page. One flask contains 5.00 g NH_3(g), and the other contains 5.00 g HCl(g). When the valve is opened, the gases react until one is completely consumed. Which gas will remain in the system after the reaction is complete? What will be the final pressure of the system after the reaction is complete? (Neglect the volume of die ammonium chloride formed.) What mass of ammonium chloride will be formed?

Explanation / Answer

Initial :
Mass of NH3 = 5 g
Molar Mass of NH3 = 17 g/mol
number of moles of NH3 = mass / molar mass = 5/17 = 0.294 mol

Mass of HCl = 5 g
Molar Mass of HCl = 36.5 g/mol
number of moles of HCl = mass / molar mass = 5/36.5 = 0.137 mol

NH3 + HCL ----> NH4Cl
Equal moles of both will react
So,0.137 mol of each will react to form 0.137 mol of NH4Cl

a)
Since number of initial moles of NH3 is more than number of moles of HCl, NH3 will remain after reaction is complete
b)
After reaction is done:
Number of moles of NH3 = 0.294 mol - 0.137 mol = 0.157 mol
Number of moles of HCl = 0
Number of moles of NH4Cl = 0.137 mol

Total number of moles, n = 0.157 mol + 0.137 mol = 0.294 mol
P = ?
V = 2 L + 2L = 4 L
T = 25 oC = (25+273) K = 298 K
use:
P*V = n*R*T
P*4 = 0.294*0.0821*298
P = 1.8 atm
Answer: 1.8 atm

c)
Number of moles of NH4Cl = 0.137 mol
Molar mass of NH4CL = 53.5 g/mol
Mass = number of moles * molar mass
            = 0.137 * 53.5
            = 7.3 g
Answer: 7.3 g

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