Part 2: Dalton's Law of Partial Pressures (section 8.8) 1. A 2.00 L container at 100. C centains 2.778 mol of H2 gas and an unknown number of moles of N2 gas. a) If the partial pressures of H2 and N2 can be denoted as PH2 and PN2 respectively, write an equation to express the total pressure (Psota) of this container. b) Use the ideal gas law equation and solve for the partial pressure of Hz gas (PH2) in this container. c) What is the partial pressure of N2 gas (PN2) in this container if Psetal is 46.6 atm?

16. The surface temperature of Venus is about 1050 K, and the pressure is about 75.0 earth atmospheres. Assuming that these conditions represent a Venusian "STP", what is the "standard" molar volume of a gas on Venus? 17. Gaseous iodine IFs can be prepared by the reaction of solid iodine and gaseous fluorine: k (s) + 5 F2 (g) → 2 IFs (g) A 5.00-L flask is charged with 10.0 g of k and 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete the temperature in the flask is 125°C. What is the partial pressure of IFs in the flask? 6.

What is the partial pressure of N₂O in a gas mixture of 15.4 g of N₂O and 6.36 g of SO₂ at a total pressure of 7.91 atm? The molar mass of N₂O is 60.02 g/mol, and the molar mass of SO2 is 64.07 g/mol. Do not put units in your answer. Record your answer to 2 decimal places.

A mixture of hydrogen and carbon dioxide gases contains hydrogen at a partial pressure of 619 mm Hg and carbon dioxide at a partial pressure of 179 mm Hg. What is the mole fraction of each gas in the mixture? X. = H₂ хсог =

1. A 2.00 L container at 100. oC contains some H2 gas and some N2 gas. a) If the partial pressures of H2 and N2 can be denoted as PH2 and PN2 respectively, write an equation to express the total pressure (Prota) of this container. (The container only has H2 gas and N2 gas) b) What is the partial pressure of N2 gas (PN2) in this container if Piotal is 46.6 atm and the partial pressure of H2 gas is 42.4 atm?

the answer for part a was 11.73. please show work for part b and explain c, thanks Calculate the pressure exerted by 17 grams of Cl2 in a 1.00 L container at 25.0 °C Report in the unit of atmospheres a. Using the ideal gas law b. Using the van der Waals equation. (Van der Waal's constants for Cl2 are a= 6.49 and b = 0.0562) c. Compare the results. (Explain on a molecular level)

Gaseous ammonia is synthesized from nitrogen and hydrogen by the reaction N2(g) + 3H2(g)→ 2NH3(g) Assume you take 355 L of H2 gas at 25.0 °C and 542 mm Hg and combine it with excess N2 gas. a )What is the theoretical yield of NH3 gas? b) If this amount of NH3 gas occupies a 125-L tank at 25.0 °C, what is its pressure?

4. A glass container was initially charged with 2.00 moles of a gas sample at 3.75 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 28.1 °C, so the final pressure in the container was reduced to 0.998 atm. Assume the volume stayed the same. How many moles of the gas sample are present at the end?