please help due tonight 3. A flask contains 0.10 mol of O2 and 0.30 mol of...
due tomorrow please help
At 298 K, a 5.0-L flask contains 0.15 mol of O, and 0.22 mol of N. Calculate the partial pressure of N2 inside the container. (note: the ideal gas constant is 0.0821 L atm/mol K) (4 points)
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...
(5 pts) A 5000. mL flask contains 600. mg of chlorine gas at a temperature of 22 °C. What is the pressure in atm inside the flask? (5 pts) A mixture of noble gases with a total pressure of 725 mm Hg at 25.0°C contains 8.86 x 103 mol Ar, 2.58 x 10-3 mol Ne and 5.84 x 10-mol Kr. Calculate the mole fraction of each gas in the mixture.
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 1.31g of N2 and 0.890g of O2 in a 1.62L container at 21 degrees celsius. Calculate the mole fraction of N2 and O2 Calculuate fhe partial pressure of N2 and O2 Hope you can help! Thank you!
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
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QUESTION 3 A container has a mix of 3 gases, totaling 1.00 mole total gas. They are He, Ar, Xe. The partial pressures of Helium is 0.467 atm, the partial pressure of Argon is 0.317 atm, the partial pressure of Xenon is 0.277 atm How many moles are helium? 2.39 x 101 mol 0.731 mol O 0.936 mol O 3.02 mol O 0 440 mol O 10 8 mol 9 89 x 10-2 mol...
At 15°C a 1.00 L container contains 9.91 mol N2 and 3.88 mol Ar. What is the partial pressure of each gas, and what is the total pressure inside the container? HOW DO WE GET THERE? What is the partial pressure of N2? atm
***Please type answer if possible*** GAS VOLUME STOICHIOMETRY PROBLEMS 1. The combustion of ethanol (C2H5OH) takes place by the following reaction equation. C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (g) What is the volume of CO2 gas produced by the combustion of excess ethanol by 23.3 grams of O2gas at 25oC and 1.25 atm? GAS VOLUME STOICHIOMETRY PROBLEMS 2. Acetic acid (CH3COOH) is formed from its elements by the following reaction equation: ...
A gas mixture contains 2.35g O2, 4.73g of F2, and 5.23g He in a 2.50L container at 65°C. Calculate the mole fraction of oxygen and the total pressure in the container.