The van der Waals parameter b is a measure of the volume excluded due to the finite size of the molecules. Estimate the size of a single molecule for: 1) Argon (Ar) b = 0.0322 L mol−1; 2) Helium (He) b = 0.0237 L mol−1; 3) Methane (CH4) b = 0.0428 L mol−1.

suppose you start with 5.000cm3 of aluminum at 21.00C. What volume would the mass of aluminum have when melted at 660.23?

If there are 1.5 x 109 cows each "passing" on the average 240. Liters of CH4 (g) per day, in one day if all of that CH4 were to be safely collected and undergo a controlled but complete combustion reaction, how many grams of CO2 would contribute to the Greenhouse effect of the Earth?   You will first need to have the combustion reaction of CH4. Make an assumption that the Temperature of the collected gas is 22.4 L = 1 mol, STP conditions (which it really is not at).

The best laboratory vacuum pump can generate a vacuum of about ∆H f olecular chlorine and molecular fluorine combine to form a gaseous product. Under the same conditions of temperature and pressure it is found that one volume of Cl2 reacts with three volumes of F2 to yield two volumes of the product. What is the formula of the product? (b) Methane, the principal component of natural gas, is used for heating and cooking. The combustion process is

HCl(g) can be made by the direct reaction of H2 and Cl2 in the presence of light. 6.00 g of H2 and 1.50 x 102 g Cl2 are mixed in a 5.00 L flask at 28.0 °C. What are the partial pressures of gases after the reaction has completed. Given Information:             > Temperature and volume remains constant at 28.0 °C             > Wavelength of light needed for the reaction is 340 nm.

A sample of 3.42 mol of xenon is confined at low pressure in a volume at a temperature of 86 °C. Describe quantitatively the effects of each of the following changes on the pressure, the average kinetic energy per molecule in the gas, and the root-mean-square speed. (a) The temperature is increased to 199 °C (b) The volume is tripled. (c) The amount of xenon is decreased to 1.87 mol Give each answer as a decimal factor of the form: new value factor old value. A factor of 1 means no change. ChangeP KEavgms

A sample of an ideal gas at 1.00 bar and a volume of 1.91 L1.91 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 60.0 bar,60.0 bar, what was the volume of the sample? Assume that the temperature was held constant.

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 550. L and heated to 520.0 °C. When the amount of CaCO3 has stopped changing, it is found that 8.46 kg have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 520.0 °C. Round your answer to 2 significant digits. P Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. 0 X

Gaseous CO exerts pressure of 45.6 mmHg in a 56.0 L tank at 22°C was released to a room with a volume of 2.70 x 104L. The room has another two gaseous that are 5.50 g of NO2 and 8.034 x 1022 atoms of SO2 at 22°C. Calculate the partial pressure of CO in the room at 22°C. •Ans : P = 0.09458 mmHg Calculate the total pressure in the room and the molarity of CO gas in the room. •Ans: 5.14 x 10-6 M, Total pressure 2,7 x 10-4 atm Calculate the density of the mixture in the room and the mass percentage of SO2 gas in the room. 6.00027

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete the lime absorbs CO₂ from the air and turns back into hard, durable 2 limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 400. L and heated to 740.0 °C. When the amount of CaCO3 has stopped changing, it is found that 3.37 kg have disappeared. P 00. Calculate the pressure equilibrium constant K this experiment suggests for the equilibrium between CaCO3 and CaO at 740.0 °C. Round your answer to 2 significant digits. Ar Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. р K₁ = 0 x10 р x Ś ? Explanation Check 0 81 K © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility