A vessel of volume 22.4 dm3 contains 2.0 mol H2(g) and 1.0 mol N2(g) at 273.15...
A vessel of volume 22.4 dm3 contains 2.0 mol H2(g) and 1.0 mol N2(g) at 273.15 K. (a) Calculate the mole fractions of each component. H2 N2 (b) Calculate the partial pressures of each component. H2 N2 (c) Calculate the total pressure.
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A vessel of volume 22.4 dm3 contains 2.0 mol H2(g) and 1.0 mol
N2(g) at 273.15...
A vessel of volume 22.4 dm3 contains 2.0 mol H2 and 1.0 mol N2 at 273.15...
A vessel of volume 22.4 dm3 contains 2.0 mol H2 and 1.0 mol N2 at 273.15 K initially. All the H2 reacted with sufficient N2 to form NH3. Calculate the partial pressures and the total pressure of the final mixture.
A gas mixture contains 0.600 mol of N2, 0.150 mol of H2, and 0.400 mol of...
A gas mixture contains 0.600 mol of N2, 0.150 mol of H2, and 0.400 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 8.00 L vessel at 27.00°C. A) What is the total pressure in the vessel (atm)? B) What is the pressure (atm) of H2? C) What is the pressure (atm) of N2? D) What is the pressure (atm) of CH4?
A gas mixture contains 0.650 mol of N2, 0.200 mol of H2, and 0.200 mol of...
A gas mixture contains 0.650 mol of N2, 0.200 mol of H2, and 0.200 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 14.0 L vessel at 27.00°C. v 4th attempt Part 1 (1 pt) X Feedback See Periodic Table D See Hint total pressure in the vessel $ 2.70 atm Part 2 (1 pt) *Feedback pressure of H2 0.560 atm Part 3 (1 pt)...
A 3.00 L flask containing 2.0 mol of O2 and 1.0 mol of N2 is in...
A 3.00 L flask containing 2.0 mol of O2 and 1.0 mol of N2 is in a room that is at 22.0˚C. a. What is the total pressure in the flask? b. What fraction of the total pressure in the flask is due to N2? c. If the temperature of the flask is lowered, what happens to the pressure inside the flask? d. On a molecular level, explain why the pressure changes as you predicted in part (c). e. If...
7. The synthesis of ammonia from the elements is conducted at high pressures and temperatures: N2(g)...
7. The synthesis of ammonia from the elements is conducted at high pressures and temperatures: N2(g) +3 H2(g) 2 NH3(g) Suppose that at one stage in the reaction, 13 mol NH3, 31 mol N2, and 93 mol H2 are present in the reaction vessel at a total pressure of 210 atm. Calculate the mole fraction of NH3 and its partial pressure.
A 22.4 L container at 0 °C contains 0.27 mol N2, 0.19 mol O2, 0.42 mol...
A 22.4 L container at 0 °C contains 0.27 mol N2, 0.19 mol O2, 0.42 mol He, and 0.050 mol CO2. What are the partial pressures of each of the gases in atm, torr, and bar
A mixture of 0.02138 mol of C2H6, 0.006096 mol of N2, 0.01567 mol of NH3, and 0.02233 mol of C2H4 is placed in a 1.0-L s...
A mixture of 0.02138 mol of C2H6,
0.006096 mol of N2, 0.01567 mol of NH3, and
0.02233 mol of C2H4 is placed in a 1.0-L
steel pressure vessel at 5155 K. The following equilibrium is
established:
3 C2H6(g) + 1 N2(g)
2 NH3(g) + 3
C2H4(g)
At equilibrium 0.0006616 mol of N2 is found in
the reaction mixture.
(a) Calculate the equilibrium partial pressures of
C2H6, N2, NH3, and
C2H4.
Peq(C2H6) = .
Peq(N2) = .
Peq(NH3) = .
Peq(C2H4)...
Exercise #1: (4 marks) Balance each of the following redox reactions in acid condition: a) Mg(s)...
Exercise #1: (4 marks) Balance each of the following redox reactions in acid condition: a) Mg(s) + H2O(g) → Mg(OH)2(s) + H2(8) b) Cr(NO3)3(aq) + Al(s) + Al(NO3)2(aq) + Cr(s) (6 marks) Exercise #2: In both cases write the balanced formula equation of the reaction and then answer to the question. a) If 25.98 mL of 0.1180 M KOH solution reacts with 52.50 mL of CH,COOH solution, what is the molarity of the acid solution? b) If 26.25 mL of...
A mixture of 0.01341 mol of CH4, 0.01170 mol of H2S, 0.02118 mol of CS2, and 0.02835 mol of H2 is placed in a 1.0-L stee...
A mixture of 0.01341 mol of CH4, 0.01170 mol of
H2S, 0.02118 mol of CS2, and 0.02835 mol of
H2 is placed in a 1.0-L steel pressure vessel at 3416 K.
The following equilibrium is established:
1 CH4(g) + 2 H2S(g) 1
CS2(g) + 4 H2(g)
At equilibrium 0.003198 mol of H2S is found in the
reaction mixture.
- Calculate the equilibrium partial pressures of CH4,
H2S, CS2, and H2.
- Calculate KP for this reaction.
1) A mixture of oxygen and ammonia at 273.15 K and 1.00 atm has a volume...
1) A mixture of oxygen and ammonia at 273.15 K and 1.00 atm has a volume of 150.0 cm .This mixture is cooled to the temperature of liquid nitrogen at which ammonia freezes out and the remaining gas is removed from the vessel. The vessel is allowed to warm to 273.15 K and 1 atm, and the volume is now 85.0 cm . Calculate the mole fraction of ammonia in the original mixture. 2) (a) Use the van der Waals...
A gas mixture contains 0.650 mol of N2, 0.200 mol of H2, and 0.200 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 14.0 L vessel at 27.00°C. v 4th attempt Part 1 (1 pt) X Feedback See Periodic Table D See Hint total pressure in the vessel $ 2.70 atm Part 2 (1 pt) *Feedback pressure of H2 0.560 atm Part 3 (1 pt)...
7. The synthesis of ammonia from the elements is conducted at high pressures and temperatures: N2(g) +3 H2(g) 2 NH3(g) Suppose that at one stage in the reaction, 13 mol NH3, 31 mol N2, and 93 mol H2 are present in the reaction vessel at a total pressure of 210 atm. Calculate the mole fraction of NH3 and its partial pressure.
A mixture of 0.02138 mol of C2H6,
0.006096 mol of N2, 0.01567 mol of NH3, and
0.02233 mol of C2H4 is placed in a 1.0-L
steel pressure vessel at 5155 K. The following equilibrium is
established:
3 C2H6(g) + 1 N2(g)
2 NH3(g) + 3
C2H4(g)
At equilibrium 0.0006616 mol of N2 is found in
the reaction mixture.
(a) Calculate the equilibrium partial pressures of
C2H6, N2, NH3, and
C2H4.
Peq(C2H6) = .
Peq(N2) = .
Peq(NH3) = .
Peq(C2H4)...
Exercise #1: (4 marks) Balance each of the following redox reactions in acid condition: a) Mg(s) + H2O(g) → Mg(OH)2(s) + H2(8) b) Cr(NO3)3(aq) + Al(s) + Al(NO3)2(aq) + Cr(s) (6 marks) Exercise #2: In both cases write the balanced formula equation of the reaction and then answer to the question. a) If 25.98 mL of 0.1180 M KOH solution reacts with 52.50 mL of CH,COOH solution, what is the molarity of the acid solution? b) If 26.25 mL of...
A mixture of 0.01341 mol of CH4, 0.01170 mol of
H2S, 0.02118 mol of CS2, and 0.02835 mol of
H2 is placed in a 1.0-L steel pressure vessel at 3416 K.
The following equilibrium is established:
1 CH4(g) + 2 H2S(g) 1
CS2(g) + 4 H2(g)
At equilibrium 0.003198 mol of H2S is found in the
reaction mixture.
- Calculate the equilibrium partial pressures of CH4,
H2S, CS2, and H2.
- Calculate KP for this reaction.
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