Question

In: Chemistry

A 5.07 g sample of water is introduced into a 0.668 L flask containing some C2H2...

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)))

Solutions

Expert Solution

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


Related Solutions

A 3.86 L flask containing 1.23 atm of Ar is connected to a 3.76 L flask...
A 3.86 L flask containing 1.23 atm of Ar is connected to a 3.76 L flask containing 1.77 atm of Kr. When the two containers are allowed to mix, (a) what is the total pressure in the containers and (b) what is the mole fraction of Ar? (a) 5.10 atm; (b) 0.415 (a) 3.00 atm; (b) 0.410 (a) 7.62 atm; (b) 0.506 none of the choices is correct
A 11.1 g sample of PCl5 is added to a sealed 1.75 L flask and the...
A 11.1 g sample of PCl5 is added to a sealed 1.75 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 49.6% of the PCl5 remains. What is the equilibrium constant, Kc, for the reaction? Equation: PCl5 (g)<----> PCl3(g) + Cl2(g)
For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55.3 at 700 K. In a 2.00-L flask containing an...
For the reaction H2(g)+I2(g)⇌2HI(g), Kc = 55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.057 g H2 and 4.39 g I2. Part A What is the mass of HI in the flask? Express your answer to two significant figures and include the appropriate units.
In the experiement, each flask containing a water sample, pipette 10.00 mL of the AgNO3 solution....
In the experiement, each flask containing a water sample, pipette 10.00 mL of the AgNO3 solution. Using a small graduated cylinder, carefully add 3.0 mL of Fe(NO3)3 solution and 2.0 mL of 6M HNO3 to each water sample. the trial is now ready for titration. Obtain approximately 120 mL of stock KSCN solution. Rinse out a clean buret with about 10 mL of KSCN at least twice, and discard the washing solution into a waste beaker.  From the calculation , number...
A 1.00 L flask is filled with 1.45 g of argon at 25 ∘C. A sample...
A 1.00 L flask is filled with 1.45 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.000 atm What is the partial pressure of argon, PAr, in the flask? What is the partial pressure of ethane, Pethane, in the flask?
A 1.00 L flask is filled with 1.20 g of argon at 25 ∘C. A sample...
A 1.00 L flask is filled with 1.20 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.450 atm . What is the partial pressure of argon, PAr, in the flask?
A 1.00 L flask is filled with 1.45 g of argon at 25 ∘C. A sample...
A 1.00 L flask is filled with 1.45 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.450 atm . What is the partial pressure of ethane, Pethane, in the flask? Express your answer to three significant figures and include the appropriate units.
A 1.10 −g sample of dry ice is added to a 765 −mL flask containing nitrogen...
A 1.10 −g sample of dry ice is added to a 765 −mL flask containing nitrogen gas at a temperature of 25.0 ∘C and a pressure of 715 mmHg . The dry ice is allowed to sublime (convert from solid to gas) and the mixture is allowed to return to 25.0 ∘C. What is the total pressure in the flask? Express your answer using three significant figures.
Mass of flask, stopper, and 5mL of water (g) 102.945 g Mass of flask, stopper, and...
Mass of flask, stopper, and 5mL of water (g) 102.945 g Mass of flask, stopper, and filled with water (g) 238.389 g Volume of gas space in flask (the difference between the above two measurements covnerted to mL) (L) .135444 L Mg(s) + HCl(aq) Reaction Trail 1 Trial 2 Mass of Mg(g) 0.008 0.007 Initial Pressure (atm) 0.9974 0.9945 Max Pressure (atm) 0.9980 0.007 Pressure Change (atm) 0.0006 0.0471 Temp (K) 295.7 296.1 a. Calculate the moles of H2 produced...
If a 1.00 L flask containing 1.00 atm of SO2 is connected to a 4.00 L...
If a 1.00 L flask containing 1.00 atm of SO2 is connected to a 4.00 L flask containing 1.00 atm of O2, and the gases are allowed to mix and react to form SO3 at 25°C, predict the total pressure (PT) in the flask after the reaction is over a. 1.10 atm b. 0.300 atm c. 0.900 atm d. 0.200 atm
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT