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 1.0 mol of H2 is added to the flask, what happens to the total pressure? What happens to the partial pressure of N2?
f. If 1.0 L is added to the original flask from part (a), how would you expect the pressure in the flask to change?
g. Which gas, N2 or O2, would you expect to have greater solubility in water? In terms of intermolecular forces, explain your answer.
Please be very specific with all the answers and explain the reasons thoroughly.
Homework Answers
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11. A 25 L flask at 25°C contains 0.75 mol of N2, 0.50 mol of O2...
11. A 25 L flask at 25°C contains 0.75 mol of N2, 0.50 mol of O2 and 1.25 mol of CO. What is the total pressure? e) 500 atm a) 0.0082 atm b) 2.4 atm c) 21 atm d) 250 atm
answer both If a 1.0 L flask is filled with 0.22 mol of N2 and 0.22...
answer both
If a 1.0 L flask is filled with 0.22 mol of N2 and 0.22 mol of O2 at 2000°C, what is (NO) after the reaction establishes equilibrium? (Kc - 0.10 at 2000°C) N2(g) + O2(8) 2NO(g) 1) 0.034 M 2) 0.060 M 3) 0.079 M 4) 0.12 M Question 34 (1 point) For the reaction of CH3NC(8) CH3CN(8) Kc = 11 What is the equilibrium concentration of CH3CN if the flask initially contains only 0.56 M CH3CN?
At 0 ⁰C, each cubic centimeter of a 1.0-L flask contains 5.0 × 10-2 mol of...
At 0 ⁰C, each cubic centimeter of a 1.0-L flask contains 5.0 × 10-2 mol of N2, 1.5 × 102 mg O2, and 5.0 × 1018 molecules of NO. What is the partial pressure of each gas, and what is the total pressure in the flask? a. 3400000 atm (total pressure) b. 1.2 atm c. 110 atm d. 1.4 atm e. 1.1 atm f. 3400000 atm g. 0.11 atm h. 1100 atm i. 1200 atm j. 0.19 atm
N2 gas in a 1.0 L tank at 1 atmosphere is transferred to a 2.0 L...
N2 gas in a 1.0 L tank at 1 atmosphere is transferred to a 2.0 L tank which already contains 2 atmospheres of O2 gas. What is the total pressure?
Suppose that Daniel has a 3.00 L bottle that contains a mixture of O2 , N2...
Suppose that Daniel has a 3.00 L bottle that contains a mixture of O2 , N2 , and CO2 under a total pressure of 5.30 atm. He knows that the mixture contains 0.310 mol N2 and that the partial pressure of CO2 is 0.350 atm. If the temperature is 273 K, what is the partial pressure of O2 ?
Ar O2 He 2.0 mol 2.0 mol 2.0 mol V = 50.0L V = 50.0 L...
Ar O2 He 2.0 mol 2.0 mol 2.0 mol V = 50.0L V = 50.0 L V = 50.0 L T= 100 K T = 500 K T = 300 K Considering the relationships summarized in the ideal gas law, in which flask is the pressure the highest? a. argon b. oxygen c. all of the gases have the same pressure d helium
For the reaction N2(g) + O2(g) 2NO(g), Kc = 4.0 at a particular temperature. In a 1.0-L...
For the reaction N2(g) + O2(g) 2NO(g), Kc = 4.0 at a particular temperature. In a 1.0-L container, 1.0 mol of N2 and O2 are mixed. Determine the concentration of NO once equilibrium is reached at the given temperature. =________ Please explain so I understand
1.0 mole of N2, 0.75 mol O2, and 0.50 mol H2, each at 25°C and 2...
1.0 mole of N2, 0.75 mol O2, and 0.50 mol H2, each at 25°C and 2 bar, are mixed isothermally. The final pressure is 2 bar. Calculate ∆S and ∆Ssurr, on the assumption of ideal behavior.
7.0 L of O2 at 1.0 atm is mixed together with 8.0 L of N2 at 7.0 atm at a constant temperature of 25 C in a 25.0 L vesse...
7.0 L of O2 at 1.0 atm is mixed together with 8.0 L of N2 at 7.0 atm at a constant temperature of 25 C in a 25.0 L vessel. What is the mole fraction of N2 in the 25.0 L vessel? Assume the gases behave ideally. Express your answer as a unitless mole fraction using at least three significant figures.
A 5.00 L flask contains 0.23 mol of oxygen. What would be the pressure in the...
A 5.00 L flask contains 0.23 mol of oxygen. What would be the pressure in the flask if 0.30 mol of carbon dioxide are added ? the temperature of the mixture is 45 C.
11. A 25 L flask at 25°C contains 0.75 mol of N2, 0.50 mol of O2 and 1.25 mol of CO. What is the total pressure? e) 500 atm a) 0.0082 atm b) 2.4 atm c) 21 atm d) 250 atm
answer both
If a 1.0 L flask is filled with 0.22 mol of N2 and 0.22 mol of O2 at 2000°C, what is (NO) after the reaction establishes equilibrium? (Kc - 0.10 at 2000°C) N2(g) + O2(8) 2NO(g) 1) 0.034 M 2) 0.060 M 3) 0.079 M 4) 0.12 M Question 34 (1 point) For the reaction of CH3NC(8) CH3CN(8) Kc = 11 What is the equilibrium concentration of CH3CN if the flask initially contains only 0.56 M CH3CN?
Ar O2 He 2.0 mol 2.0 mol 2.0 mol V = 50.0L V = 50.0 L V = 50.0 L T= 100 K T = 500 K T = 300 K Considering the relationships summarized in the ideal gas law, in which flask is the pressure the highest? a. argon b. oxygen c. all of the gases have the same pressure d helium
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