B. In the following graphs, velocity represents the molecular speed,Velocity (m/s)(i)If the plot represents the velocity distribution of 1.0 L of O2 (g) at temperature of 2273 Kversus 127 K, which plot corresponds to each temperature? Briefly explain(ii)If the plot represents the velocity distribution of 1.0 L of He (g) at STP and 1.0 L of Cl, (g)at STP, which plot corresponds to which gas? Briefly explain.C. Calculate the molar mass of a gas X2 if equal volumes of X2 and hydrogen gas take 9.12 and1.20 minutes, respectively, to effuse into a vacuum through a small hole under the same conditions ofconstant pressure and temperature.Relative number of molecules

Ideal gases are hypothetical gases which do have real existence. A gas can behave ideally at low…

B. In the following graphs, velocity represents the molecular speed, Velocity (m/s) (i) If the plot represents the velocity distribution of 1.0 L of O2 (g) at temperature of 2273 K versus 127 K, which plot corresponds to each temperature? Briefly explain If the plot represents the velocity distribution of 1.0 L of He (g) at STP and 1.0 L of Cl2 (g) (ii) at STP, which plot corresponds to which gas? Briefly explain. Relative number of molecules

B. In the following graphs, velocity represents the molecular speed, Velocity (m/s) (i) If the plot represents the velocity distribution of 1.0 L of O2 (g) at temperature of 2273 K versus 127 K, which plot corresponds to each temperature? Briefly explain If the plot represents the velocity distribution of 1.0 L of He (g) at STP and 1.0 L of Cl2 (g) (ii) at STP, which plot corresponds to which gas? Briefly explain. Relative number of molecules

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

1. Calculate the density of oxygen, O2, under each of the following conditions: STP 1.00 atmatm and 10.0 ∘C 2. To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 3.8-L bulb, then filled it with the gas at 1.70 atm and 20.0 ∘C and weighed it again. The difference in mass was 7.5 g . Identify the gas. Express your answer as a chemical formula.
Consider the following reaction for the combustion of octane, C8H18: 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H20(l) What volume of oxygen gas at STP would be needed for the complete combustion of 33.0 g of octane?
In Dalton's Law of Partial Pressures: Ptrapped gas = Pdry gas + Pwater vapor Why must the pressure of water vapor be included in this calculation? a. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater vapor has to be added to Pdry gas. b. Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. c. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. d. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor.
11. Consider the following chemical reaction: CO2(g) + NaOH(aq) ---------> Na2CO3(s) + H2O(l) CO2(g) + KOH(aq) --------> K2CO3(s) + H2O(l) Carbon dioxide gas is bubbled into a 2.50 L. flask contains mixture of sodium hydroxide and potassium hydroxide. After evaporation of water and drying the mass of the residues is 14.5 g. Calculate grams of sodium hydroxide in the mixture. The pressure of carbon dioxide gas is 855 mmHg and the temperature is 25 oC. Na = 22.99 g/mole, K = 39.10 g/mole, H= 1.008 g/mole, O = 16.00 g/mole, C = 12.01 g/mole a.8.88 gb.1.19 gc.2.34 gd.3.48 g
Ethane burns in air to give h2o and o2 . 2c6h6+ 7o2= 4co2+ 6h2o What volume of o2 (L) is required for complete reaction with 6.8 L of c6h6 ? Assume all gases are measured at the same temperature and pressure. Volume = __L What volume of h2o vapor (L) is produced in the complete reaction of 6.8 L of c6h6 ? Assume all gases are measured at the same temperature and pressure. Volume =___ L
A prototype sports ball for a new game is precisely inflated to a pressure of 7.3 psi at 25 degrees C. The ball is spherical with an inner bladder diameter of 22.8 cm. It is filled with air (Mw=28.97 g/mol). Not Avogadro’s number is 6.022 x 10^23 atom/mol. A. Calculate the number of moles of air in the ball at the specified temperature and pressure. Consider the air in the ball to follow the ideal gas law. PV=nRT Where P is the absolute pressure of the air in atm, V is the volume of the ball, T is the absolute temperature in K, and R is the ideal gas constant. B. How many oxygen atoms compose the air in the ball? Assume that the mole fraction of N2 in the air is 0.79 and the remainder of the air is 02(oxygen).
7.) A glass bulb contains an unknown gas. The gas is either CO2, SO2, C2H6, or CH3F. Here is some data that was collected for this gas sample. Use the data to identify the unknown gas. Mass of glass bulb with the unknown gas: 14.402 g Volume of glass bulb: 670. mL Mass empty bulb 12.232 g Pressure 1751. torr Temperature 21.oC
Calculate the partial pressure of helium gas for a volume of 1.0 x 10-° m³ of 20°Rn gas after 14 minutes. The radon gas was originally placed in an evacuated container at 1 atm, and the temperature remains constant at 0°C. (t, 12 = 5.67 min for 20°Rn.) 0.18 X atm What is the partial pressure of the radon gas after this time? atm
A 22.5 mL sample of liquid ethanol (C₂H₅OH, density = 0.789 g/mL) was injected into a 10.0 L cylinder containing O₂ at a pressure of 4.50 atm and a temperature of 25°C. The cylinder was heated to 125°C and a spark was used to ignite the ethanol, which was completely combusted. What was the final total pressure in the cylinder (in atm) after the reaction, while it was still at 125°C?
Charles' Law explores the effects of temperature on the volume of an ideal gas. Charles’ Law is described as V₁/T₁ = V₂/T₂. A gas with an initial volume of 2.00 L at 275.0 K is heated. The final volume is 3.0 L. Calculate the final temperature of the gas, in K.
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.
Butane, CAH10, is an easily liquefied gaseous fuel. Calculate the density of butane gas at 0.857 atm and 22 °C. Give the answer in grams per liter. Given that R = 0.0821 L-atm/(mol-K), AW of C = 12.01 amu, and AW of H = 1.01 amu. a. 1.83 g/L. O b. 2.08 g/L. O c. 1.56 g/L. o d. 1.35 g/L. O e. 2.32 g/L.