In: Chemistry
A 5.07 g sample of water is introduced into a 0.668 L flask
containing some C2H2 gas. The flask is heated
to 233.53 °C at which temperature all of the water is converted to
the gaseous phase, giving a total pressure in the flask of 20.932
atm.
1. Calculate PH2O (in atm) in the flask at
233.53 °C.
Report your answer to **((three
decimal places)) in standard notation (i.e. 1.234 atm).
2-Calculate PC2H2 (in atm) in the flask at 233.53
°C.
Report your answer to**((( three
decimal places)) in standard notation (i.e. 1.234 atm)
3. Calculate the mass of C2H2 (in grams)
in the flask at 233.53 °C.
Report your answer to ***(((three
significant figures.)))
4. Calculate XH2O in the flask at 233.53
°C.
Report your answer to ***(((three
significant figures)))
Solution :-
1. Calculate PH2O (in atm) in the flask at 233.53
°C.
Report your answer to **((three decimal places)) in standard
notation (i.e. 1.234 atm).
Solution :-
Lets first calculate the moles of water
Moles of water = 5.07 g /18.0148 g per mol = 0.28144 mol
Now we can calculate the pressure of the H2O using the ideal gas law formula
V= 0.668 L
T= 233.53 +273.15 = 506.68 K
PV=nRT
P =nRT/V
= 0.28144 mol * 0.08206 L atm per mol K * 506.68 K / 0.668 L
= 17.518 atm
So the partial pressure of the H2O = 17.518 atm
2-Calculate PC2H2 (in atm) in the flask at 233.53
°C.
Report your answer to**((( three decimal places)) in standard
notation (i.e. 1.234 atm)
Solution :-
P C2H2 = total pressure - P H2O
= 20.932 atm – 17.518 atm
= 3.414 atm
3. Calculate the mass of C2H2 (in grams)
in the flask at 233.53 °C.
Report your answer to ***(((three significant figures.)))
Solution :-
Lets calculate the moles of the C2H2 using the ideal gas formula
n= PV/RT
= 3.414 atm* 0.668 L / 0.08206 L atm per mol K * 506.68 K
= 0.05485 mol C2H2
Now lets calculate the mass of C2H2
Mass of C2H2 = moles * molar mass
= 0.05485 mol * 26.04 g per mol
= 1.43 g C2H2
4. Calculate XH2O in the flask at 233.53 °C.
Report your answer to ***(((three significant figures)))
Solution :-
Mole fraction can ce calculated using the partial pressure and total pressure as follows
XH2O = P H2O / total pressure
= 17.518 atm / 20.932 atm
= 0.837