What is the ratio of urms to ump for a sample of O21g2 at 300 K? Will this ratiochange as the temperature changes? Will it be different for a different gas?

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 5.80 g sample of lead nitrate Pb(NO3)2 molar mass = 331 g/mol is heated in an evacuated cylinder with a volume of 3.25L. The salt decomposes when heated according to the equation: 2Pb(NO3)2 --> 2PbO + 4NO2 + O2 Assuming complete decomposition, what is the pressure in the cylinder after decomposition and cooling to a temperature of 250 K?

5.(a) Assume for the moment that air consist of 80.00% nitrogen and 20.00% oxygen byvolume. Use these figures and typical values for temperature and pressure (1.000atm, 25.0 ºC) to calculate the density of air. (b) This calculation affords a good approximation of the density of air at sea level.However, your lab is at an altitude approximately 777 meters (2550 feet). Knowingthis, will the density of air in you lab be higher or lower than the value you justcalculated? Why? (c) Besides altitude, what else affects the atmospheric pressure? Where could you findthe actual atmospheric pressure at the time of the experiment?

Combustion of hydrocarbons such as pentane (C5H12) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. A.) suppose 0.100 kg of pentane are burned in air at a pressure of exactly 1 atm and a temperature of 13°C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to three significant digits.

Consider a sample of a hydrocarbon (a compound consisting of only carbon and hydrogen) at 0.959 atm and 298 K. Upon combusting the entire sample in oxygen, you collect a mixture of gaseous carbon dioxide and water vapor at 0.755 atm and 375 K. This mixture has a density of 0.6955 g/L and occupies a volume eight times as large as that of the pure hydrocarbon under initial conditions. Determine the molecular formula of the hydrocarbon. (Enter the elements in the order: C, H.) Molecular formula: Submit Answer Try Another Version 3 item attempts remaining

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The ideal gas law, PV = nRT is independent of the kind of gas. In other words, the pressure exerted by a given number of ideal gas particles is the same whether the sample consists of all one type of particle or a mixture of different kinds of particles. Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules. Therefore, the pressure exerted by a mixture of gases can be expressed as follows: Part A Tota RT Ptotal = V What is the partial pressure of nitrogen in air at atmospheric pressure (101 kPa)? Assume ideal behaviour. A partial pressure is the pressure exerted by just one type of gas in a mixture. A partial pressure is calculated using only the number of moles of that particular gas, instead of the total number of moles: Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) RT P = V P = nRT P= nRT etc. The sum of the partial pressures is equal to the total…

19. A 2.00 liter of sample of ethane, C;H6, is burned at 1.00 atm and 25.0 °C with 1.50 liters of oxygen. What is the mass of water vapor will be produced from the burning of ethane? What would be the volume of the water vapor under the same conditions? (Hint: determine the limiting reagent!) (m = 1.96 g; v = 1.29 L.