Answer:
5.06 atm
Step-by-step explanation:
Step 1:
Data obtained from the question. This includes:
Mass of S2O = 175g
Volume (V) = 16600 mL
Temperature (T) = 195°C
Pressure (P)
Step 2:
Determination of the number of mole of S2O in 175g of S2O.
Mass of S2O = 175g
Molar Mass of S2O = (32x2) + 16 = 64 + 16 = 80g/mol
Number of mole of S2O =.?
Number of mole = Mass/Molar Mass
Number of mole of S2O = 175/80
Number of mole of S2O = 2.1875 moles
Step 3:
Conversion to appropriate units.
It is essential to always express the various variables in the right units of measurement in order to obtain the desired answer in the right units.
For volume:
1000mL = 1L
Therefore, 16600mL = 16600/1000 = 16.6L
For temperature:
Temperature (Kelvin) = temperature (celsius) + 273
Temperature (celsius) = 195°C
Temperature (Kelvin) = 195°C + 273 = 468K
Step 4:
Determination of the pressure.
The pressure can be obtained by the application of the ideal gas equation. This is illustrated below:
Volume (V) = 16.6L
Temperature (T) = 468K
Number of mole (n) = 2.1875 moles
Gas constant (R) = 0.082atm.L/Kmol
Pressure (P) =
PV = nRT
P x 16.6 = 2.1875 x 0.082 x 468
Divide both side by 16.6
P = (2.1875 x 0.082 x 468) /16.6
P = 5.06 atm
Therefore, the pressure is 5.06 atm