Question
In: Chemistry
Part A A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at...
Part A
A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 25.0 ∘C is 2.05 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask?
Express your answer to three significant figures and include the appropriate units.
Part B
If 1.00 mol of argon is placed in a 0.500-L container at 28.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)?
For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol.
Express your answer to two significant figures and include the appropriate units.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
Part A: A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at...
Part A: A 3.00-L flask is filled with gaseous ammonia, NH3. The
gas pressure measured at 25.0 ∘C is 1.15 atm . Assuming ideal gas
behavior, how many grams of ammonia are in the flask?
Part B If 1.00 mol of argon is placed in a 0.500-L container at
20.0 ∘C , what is the difference between the ideal pressure (as
predicted by the ideal gas law) and the real pressure (as predicted
by the van der Waals equation)?
For...
1)A completely empty 2.00 L reaction vessel is filled with ammonia gas (NH3) at a constant...
1)A completely empty 2.00 L reaction vessel is filled with
ammonia gas (NH3) at a constant temperature of 680K. The
initial partial pressure of NH3 was 9.40 atm. With time
it partially decomposed according to the reaction below until
equilibrium was reached:
2 N H 3 ( g ) ⟺ 3 H 2 ( g ) + N 2 ( g )
At equilibrium the total pressure inside the flask was 12.80
atm. What is the equilibrium partial pressure of...
A 2.50 L container is filled with gaseous H2S at 13.0ºC and a pressure of 169.1...
A 2.50 L container is filled with gaseous H2S at 13.0ºC and a
pressure of 169.1 torr. Then 200.0 mL of water is added to the
container (without allowing any of the H2S to escape). A small
amount of H2S dissolves in the water. When the system has reached
equilibrium, the gas pressure in the container is 155.9 torr and
the temperature is still 13.0ºC. The vapor pressure of water at
this temperature is 11.2 torr. What is the molar...
A flask is filled with 4.0 atm of gaseous H2 and 3.0 atm of gaseous N2....
A flask is filled with 4.0 atm of gaseous H2
and 3.0 atm of gaseous N2. When a lit match is thrown
into the flask, the gases react and form gaseous NH3.
What is the pressure in the flask after the reaction?
Answer: 4.33 atm.
Please provide step by step on how to
solve.
A sample of 7.80 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is...
A sample of 7.80 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is
bubbled into a 0.250 L solution of 0.400 M HCl
(hydrochloric acid). The Kb value for NH3 is 1.8×10−5
.
Assuming all the NH3 dissolves and that the volume of the
solution remains at 0.250 L , calculate the pH of the resulting
solution.
Express your answer numerically to two decimal places.
A sample of 7.50 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is...
A sample of 7.50 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is
bubbled into a 0.350 L solution of 0.400 M HCl (hydrochloric
acid).
The Kb value for NH3 is 1.8×10−5.
Assuming all the NH3 dissolves and that the volume of the
solution remains at 0.350 L , calculate the pH of the resulting
solution.
A sample of 7.60 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is...
A sample of 7.60 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is
bubbled into a 0.450 L solution of 0.400 M HCl (hydrochloric acid).
The Kb value for NH3 is 1.8×10−5.
Part A
Assuming all the NH3 dissolves and that the volume of the solution
remains at 0.450 L , calculate the pH of the resulting solution.
Express your answer numerically to two decimal places.
A sample of 7.80 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is...
A sample of 7.80 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is
bubbled into a 0.500 Lsolution of 0.400 M HCl
(hydrochloric acid).
The Kb value for NH3 is 1.8×10−5. Assuming all the NH3
dissolves and that the volume of the solution remains at 0.500 L ,
calculate the pH of the resulting solution.
A sample of 7.70 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is...
A sample of 7.70 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is
bubbled into a 0.400 L solution of 0.400 M HCl (hydrochloric acid).
The Kb value for NH3 is 1.8×10−5.
Assuming all the NH3 dissolves and that the volume of the
solution remains at 0.400 L , calculate the pH of the resulting
solution. Express your answer numerically to two decimal
places.
1) What is the pressure in a 18.2-L cylinder filled with 27.0g of oxygen gas at...
1) What is the pressure in a 18.2-L cylinder filled with 27.0g
of oxygen gas at a temperature of 329K ?
2) A gas mixture with a total pressure of 765mmHg contains each
of the following gases at the indicated partial pressures: CO2,
129mmHg ; Ar, 208mmHg ; and O2, 191mmHg . The mixture also contains
helium gas.
What mass of helium gas is present in a 12.4-L sample of this
mixture at 276K ?
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