Tutored Practice Problem 10.4.1 COUNTS TOWARDS GRADE Calculate pressure using Dalton's law of partial pressures. Close Problem A gas mixture is made up of N2 (9.74 g), He (1.03 g), and O2 (12.6 g). The mixture has a volume of 27.6 L at 38 °C. Calculate the partial pressure of each gas in the mixture and the total pressure of the gas mixture. P N₂ He 02 = atm = atm = atm atm Ptotal Check & Submit Answer Show Approach

Calculate U when 1.00 mol of H2 goes from 1.00 atm, 10.0 L, and 295 K to 0.793 atm, 15.0 L, and 350 K.

Consider the following sketch. Each square in bulb A represents a mole of atoms X. Each circle in bulb B represents a mole of atoms Y. The bulbs have the same volume, and the temperature is kept constant. When the valve is opened, atoms of X react with atoms of Y according to the following equation: 2X(g)+Y(g)X2Y(g)The gaseous product is represented as and each represents one mole of product. (a) IfP A=2.0 atm, what is P8 before the valve is opened and the reaction is allowed to occur? What is P A+P B? (b) Redraw the sketch to represent what happens after the valve is opened. (c) What is PA? What is PB? What is P A+P B? Compare your answer with the answer in part (a).

References Use the References to access important values if needed for this question. A mixture of nitrogen and carbon dioxide gases contains nitrogen at a partial pressure of 588 mm Hg and carbon dioxide at a partial pressure of 294 mm Hg. What is the mole fraction of each gas in the mixture? XN, = Xco, = Submit Answer

Conceptual Connection 10.5 Enhanced with Feedback A gas mixture contains an equal number of moles of He and Ne. The total pressure of the mixture is 6.0 atm. Part A What are the partial pressures of He and Ne? O PHe = 4.0 atm; PNe 2.0 atm PHe = 3.0 atm; PNe = 3.0 atm O PHe = 2.0 atm; PNe 4.0 atm

10 mol of NH3 (g) were placed in a previously evacuated 20-L container.  After a sudden temperature rise to 961.4 K, 80% of ammonia dissociated into hydrogen and nitrogen according to the reaction: 2/3 NH3 (g) --> 1/3 N2 (g) + H2 (g)    What is the total pressure of the mixture if all gases are ideal? (Answer in sig figs)

= O Gases Calculating partial pressure in a gas mixture tab sulfur tetrafluoride E.H chlorine pentafluoride Explanation A 8.00 L tank at 29.8 °C is filled with 14.2 g of sulfur tetrafluoride gas and 13.7 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. Esc Check 1 Type here to search Total pressure in tank: F1 mole fraction: partial pressure: Q mole fraction: partial pressure: @ 2 F2 W F3 # 3 E J 0 0 atm 0 0a 9x atm atm F4 $ 4 R FS TI X F % 012 5 50% T F6 3 A 6 G F7 Y & 7 H FB * 8 athenaCollector v2. 4 4 J FO © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 57°F Cloudy ^ 40 10:31 AM 11/13/2023 O ( prt sc 9 F10 5 home athenaCollector v2... O K F11 OI 1/5 end F12 P D 3 Danasia V All Booken insert = ? alo Ar back

А vessel containing Ne(g) and Ar(g) has a total pressure of 9.78.  If the partial pressure of the Neon (PNe) is 3.78 and the partial pressure of the ARgon (PAr) is 6.00 , then the mole-fraction of Ne(g) is_____ and the mole fraction of Ar(g) is ____ ?

Required information Problem 13.012 - DEPENDENT MULTI-PART PROBLEM - ASSIGN ALL PARTS NOTE: This is a multi-part question. Once an answer is submitted, you will be unable to return to this part. A gas mixture consists of 2 kg of O2, 3 kg of N2, and 5 kg of CO2. Problem 13.012.c Molar Mass and Gas Constant Determine the average molar mass and gas constant of the mixture. The universal gas constant is Ru= 8.314 kJ/kmol-K. The average molar mass is kg/kmol. The gas constant of the mixture is kJ/kg-K.