If standard atmospheric pressure is 14.7ln/in^2, calculate what a pressure of 1.72lb/in^2 would be in mm Hg

A scuba diver’s tank contains 0.30 kg oxygen (O2) compressed into a volume of 2.32 L.(a) Use the ideal gas law to estimate the gas pressure     inside the tank at 5°C, and express it in atmospheres     and in pounds per square inch.(b) What volume would this oxygen occupy at 30°C and      a pressure of 0.98 atm?

At 287 K and 1.43*10^-2 atm, the density of a gas is 1.37*10^-5 g/cm^3. (a) Find the Vrms for the gas molecules. (b) Find the molar mass of the gas.

5.69 You want to store 165 g of CO2 gas in a 12.5-L tank at room temperature (25°C). Calculate the pressure the gas would have using (a) the ideal gas law and (b) the van der Waals equation. (For CO2, a = 3.59 atm L^2/mol^2 and b = 0.0427 L/mol.)

When collecting a gas over water it is necessary to correct for the vapor pressure of water in order to determine the pressure of the gas you are collecting. We will do this by using a graph of ln P in mmHg versus 1/T where T is the temperature in Kelvin. The equation is y = -5206.4 x + 20.621 (With an R^2 = 0.9999). If you collect a gas at 26.8 ℃, what is the value of “x” that you want to use in the equation. (Keep the answer for the next question). (Keep extra digits, you do not want to round in the middle of this calculation). Select one:   a. 0.003660992 b. 0.037313433 c. 0.003378378 d. 299.95 e. 0.0273150 f. 273.15 g. None of these h. 0.003333889 i. 0.0027315

11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b)  The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.

The critical pressure, Pe, and the critical temperature, Te, of gas A are 3.040 × 10° Pa and 473 K, respectively. (i) Calculate the van der Waals constants, a and b, for this gas. (ii) Gas A obeys the van der Waals equation. Calculate the pressure exerted by one mole of gas A if the molar volume occupied by this gas is 2.75 L/mol at 298 K.

Q1 (a) 3.2 g of sulphur was produced in a reaction between 6.0 L of hydrogen sulfide gas with excess an amount of sulphur dioxide. With the aid of Table Q1 (a)(i) and Table Q1 (a)(ii), predict the temperature (in °C) of the reaction if it was conducted at 750 torr. Element Actinium Aluminum Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Boron Bromine Cadmium Calcium Californium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Curiam CY с Ce Cs a Cr Co Ca Cm Dysprosium Dy Einsteinium Es Er Eu Fm F Fr Gd Ga Ge Erbium Europium Fermium Fluorine Francium Gadoliniam Gallium Germaniam Gold Hafnium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanam Lawrencium Lead Lithiam Lutetium Table Q1 (a)(i): Atomic Number and Atomic Mass of Elements Magnesium Manganese Symbol Ac Al Am Sb As Al Ba Bk Be Bi B Br Ca Hr He Ho H In I Ir Fe Kr La Lr Ph Li Lu Mg Mn Atomic number (2) 89 13 95 51 18 33 85 56 97 4 83 5 35 48 20 98 6 58 55 17 24 27 29 96 66 99 68…

For many purposes we can treat ammonia (NH,) as an ideal gas at temperatures above its boiling point of –33. °C. Suppose the temperature of a sample of ammonia gas is raised from – 25.0 °C to 17.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.15 kPa and the volume decreased by 50.0%, what is the final pressure? Round your answer to 2 significant digits. kPa 1 Don't Know Submit etv DII esc %23 24 6 7 09 2 4 OP E T Y.

73. A 500.-mL sample of O2 gas at 24 °C was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2 O2, in the presence of a small amount of manganese catalyst by the reaction 2H2 O2 (aq) → 2H2O (g) + The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? (The vapor pressure of water at 24 °C is 23 mm Hg.)