What is the total pressure in a 9.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of...
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
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?
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
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...
A 7.75-L flask contains 0.482 g of hydrogen gas and 4.98 g of oxygen gas at 65°C. What is the partial pressure of oxygen in the flask? Multiple Choice Ο 0.557 atm Ο 0.043 atm Ο 33.5 atm Ο 67 atm Ο 1.11 atm < Prev 15 of 26 !! Next >
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 50.0 L gas mixture at T = 500 K contains 123.0 g H2 and 855.0 g CO. What is the total pressure of the mixture? Assume ideal-gas behavior. Molar masses: M(H2) = 2.016 g/mol, M(CO) = 28.01 g/mol. (A) 116 atm (B) 75.1 atm (C) 50.1 atm (D) 34.1 atm (E) 25.0 atm
A flask contains 1.00 L of a pure gas at 0.850 atm and 20.0°C. The mass of the gas is 1.13 g. a) What is the molar mass of the gas? (use the correct sig. fig as well as the units b) What is its identity? arades eople A mixture of gases containing 21.0 g of N2, 106.5 g of Cly, and 120 g of He at 14 °C is in a 50.0L container. What is the total pressure in...
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.
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.