Solution:
According to ideal gas equation for Cl2 gas,
PV = n R T
n = PV /RT
Where,
n= number of mol = ?
P = pressure = 805 torr / 760 = 1.06 atm
V = volume = 295 mL = 0.295 L
R = 0.0821 L atm K-1 mol-1
T = 25 + 273 = 298 K
Thus,
n = 1.06 atm x 0.295 L / 0.0821 L atm K-1 mol-1 x 298 K
n = 0.01278 mol of Cl2
From the given reaction, it can be seen that 1 mol Cl2 is produces from 1 mol MnO2
Thus, 0.01278 mol Cl2 produces from 0.01278 mol of MnO2.
Hence,
Mass of MnO2 = number of mol x molar mass
= 0.01278 mol x 86.9368 g mol-1 = 1.11 g
Question 13 of 13 Chlorine can be prepared in the laboratory by the reaction of manganese...
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Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl ( aq ) , as described by the chemical equation MnO 2 ( s ) + 4 HCl ( aq ) ⟶ MnCl 2 ( aq ) + 2 H 2 O ( l ) + Cl 2 ( g ) How much MnO 2 ( s ) should be added to excess HCl ( aq ) to obtain 215 mL Cl 2...
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