Calculate the root-mean-square velocity, in m/s, for a hydrogen molecule at -17.0 °C. The universal gas constant, R=8.314 J/mol·K.

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

An experiment is performed to determine the volume of gas produced by the following reaction: 2HCl(aq) + Mg­(s)                  MgCl2(aq) + H2(g) A.  What is the maximum mass of Mg in g that could be reacted at 20oC temperature and 1.0atm, if the volume of the gas burette is 50mL? (Hint: Find moles of H2 using the ideal gas law; then, convert to g of Mg.)   B. If the experiment were moved to a higher elevation and the pressure was decreased to 0.95 atm would the maximum amount of Mg increase or decrease?   C. If 16mg of Mg were reacted, what is the volume of gas produced in this reaction?   D. What is the solvent for this reaction?   E. Would the HCl(aq) be considered a strong, weak, or non-electrolyte?   F. Would the MgCl2(aq) be considered a strong, weak, or non-electrolyte?

A 1.00 LL flask is filled with 1.20 gg of argon at 25 ∘C∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.350 atmatm . part A: What is the partial pressure of argon, PArPAr Part B: What is the partial pressure of ethane, PethanePethane

A particular balloon can be stretched to a maximum surface area of 1257 cm². The balloon is filled with 3.2 L of helium gas at a pressure of 759 torr and a temperature of 310 K. The balloon is then allowed to rise in the atmosphere. Assume an atmospheric temperature of 273 K and determine at what pressure the balloon will burst. (Assume the balloon to be in the shape of a sphere.) Express your answer using two significant figures. 15] ΑΣΦ P = 0.22 Submit Previous Answers Request Answer ? X Incorrect; Try Again; 5 attempts remaining atm

The van der Waals constants for HCl are a = 3.67 atm·liter2·mole–2, and b = 40.8 cc·mole–1. Find the critical constants of this substance.

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 a limekiln of volume 800. L is pressurized with carbon dioxide gas to 14.9 atm, and heated to 960.0 °C. When the amount of CO, has stopped changing, it is found that 3.96 kg of CaCO, have appeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 960.0 °C. Round your answer to 2 significant digits. 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. K = 3.07 P

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

The air pollutant NO is produced in automobile engines from the high-temperature reaction: N₂(g) + O2(g) = 2 NO(g) K 1.7 x 103 at 2300 K.

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