1st calculate moles of CO2 formed
we have:
P = 350.0 mm Hg
= (350.0/760) atm
= 0.4605 atm
V = 25.0 mL
= (25.0/1000) L
= 0.025 L
T = 25.0 oC
= (25.0+273) K
= 298 K
find number of moles using:
P * V = n*R*T
0.4605 atm * 0.025 L = n * 0.08206 atm.L/mol.K * 298 K
n = 4.706*10^-4 mol
from reaction,
moles of HC3H3O3 reacting = moles of CO2 formed
= 4.706*10^-4 mol
Molar mass of HC3H3O3 = 3*MM(H) + 3*MM(C) + 3*MM(O)
= 3*1.008 + 3*12.01 + 3*16.0
= 87.054 g/mol
we have below equation to be used:
mass of HC3H3O3,
m = number of mol * molar mass
= 4.706*10^-4 mol * 87.054 g/mol
= 4.10*10^-2 g
Answer: 4.10*10^-2 g
Feel free to comment below if you have any doubts or if this answer do not work
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