Given:
P = 715.0 torr
= (715.0/760) atm
= 0.9408 atm
V = 335.0 mL
= (335.0/1000) L
= 0.335 L
T = 25.0 oC
= (25.0+273) K
= 298 K
find number of moles using:
P * V = n*R*T
0.9408 atm * 0.335 L = n * 0.08206 atm.L/mol.K * 298 K
n = 1.289*10^-2 mol
From reaction,
Mol of MnO2 required = mol of Cl2 produced
= 1.289*10^-2 mol
Molar mass of MnO2,
MM = 1*MM(Mn) + 2*MM(O)
= 1*54.94 + 2*16.0
= 86.94 g/mol
use:
mass of MnO2,
m = number of mol * molar mass
= 1.289*10^-2 mol * 86.94 g/mol
= 1.121 g
Answer: 1.12 g
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