13.22 grams of the gas X2 are placed in a sealed container at 35.0°C with 15.99 grams of the gas T2. The tot pressure in the container is 356.2 mmHg. (a) Find the mole fraction of T2 (b) Find the percent of T2 (c) Find the partial pressure of T2 in mmHg (PH2) Molar Mass: X: 45.65 g/mol T: 89.52 g/mol

13.22 grams of the gas X2 are placed in a sealed container at 35.0°C with 15.99 grams of the gas T2. The tot pressure in the container is 356.2 mmHg. (a) Find the mole fraction of T2 (b) Find the percent of T2 (c) Find the partial pressure of T2 in mmHg (PH2) Molar Mass: X: 45.65 g/mol T: 89.52 g/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

low-up and reports 360° reports More - Ideal Gas Law v Accessibility Mode 5. What pressure, in atmospheres, will be exerted by 0.5 moles of a gas contained in a 2.4 Liter container at 45°C? 6. How many moles of gas will a 250 ml flask hold at 87°C and950 mmHg?
1.) Calcium hydride (CaH2) reacts with water to form hydrogen gas: CaH2 (s) + 2H2O (I) ---> Ca(OH)2 (aq) + 2H2 (g) How many grams of CaH2 are needed to generate 48.0 L of H2 gas at a pressure of 0.992 atm and a temperature of 32oC?
The following system is used for q7-q9 10.00g of O2 and 15.00g N2 are combined in a 20.0L container at 25.00oC O2 32.00g/mol N2 28.02 g/mol R= 0.08206 L atm/mol K What is the partial pressure (atm) of the N2 in the container above. (3 sig figs)
As in the following equation: 802(9) 850 2(g) -> When 64.0 g S, reacted, What is the volume (L) of SO, gas produced under 802 mmHg at 33 oC. Choose... Choose... 37.6 47.5 1.81 0.271 0.80 A mixture of 5.65 g N, and 5.00 g O, has a total pressure of 0.621 atm. Calculate the partial pressure of 0, in (atm) 0.237 400 32.0 100 A sample of nitrogen gas has a volume of 22.4 L at 20.0 °C. The gas is heated to 146 °C at consant pressure. What is the final volume ( in liters) of nitrogen gas? Choose... A sample of an ideal gas had its volume doubled while its temperature remained constant, if the original pressure was 200 torr, what is the new pressure ( in torr) Choose... Assuming ideal gas behavior, what is the density in gIL of unknown gas X, which has molar mass 18.0 g/mol at STP? Choose... v
1) If 4.21 L of NH3 at 27 °C and 1.02 atm is combined with 5.35 L of HCl at 26 °C and 0.998 atm. (R 0.082 L'atm/K mol) (10 pts) %3D NH3 + HCI NHẠC1 A) Which gas is the limiting reactant? B) What mass of NH,Cl (s) will be produced? 2) What volume of 0.305 M AGNO; is required to react exactly with 155.0 mL of 0.274 M DELL
You want to prepare some oxygen gas in the laboratory using the following reaction: 2KClO3(s) --> 2KCl(s) + 3O2(g) How many liters of the oxygen gas will you collect at 1.00 atm and 22.0oC when you heat 5.05 g of potassium chlorate, KClO3 (molar mass = 122.55 g/mol), but only 85.0% of the compound completely decomposed? (A) 0.112 L (B) 1.50 L (C) 1.27 L (D) 0.998 L
Consider the following reaction: 2CuCl2 (s) → 2CUCI + Cl2 (e) An initial mass of CuCl2 (mol. wt. 134.4 g/mol) is reacted to produce Cl2 gas. The final volume of gas collected after the reaction is 2.46 L. The temperature is 300K and the pressure 1 atm. How many grams of CuCl, were reacted? O 14.2 g O 7.09 g 26.9 g O 6.72 g O 13.4 g « Previous
What is the molar mass (in g/mol) of a gas if it has a density of 1.75 g/L at a pressure of 742 mm Hg and a temperature of 22.0°C?
A student inflates a ballon to a volume of 972 mL by filling it with Argon gas at a pressure of 1.50 atm and a temperature of 15.8 C. How many grams of argon gas are neeeded? What is the partial pressure of oxygen in a container that contains 6.22? Mol to oxygen, 4.34 mol of nitrogen, and 2.39 mol of carbon dioxide when the total pressure is 817 mm Hg?
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?
help with this factors
What pressure will be exerted, in kPa, by 0.200 moles of carbon dioxide gas with a volume of 0.500 L at a temperature of 27°C? (Number only, no units) Blank 1: