A sample of neon gas is held in a rigid 6.351L container with a pressure of 1.026 atm at 22.9°C. 8.441g of an unknown cold gas is added to the container. The temperature drops to 19.8°C, but the pressure rises to 1.856atm. What is the molar mass of the added gas? [Hint: You know P, V, and T for the neon. Use this to calculate the number of moles of neon which doesn't change when the new gas is added.]

A sample of neon gas is held in a rigid 6.351L container with a pressure of 1.026 atm at 22.9°C. 8.441g of an unknown cold gas is added to the container. The temperature drops to 19.8°C, but the pressure rises to 1.856atm. What is the molar mass of the added gas? [Hint: You know P, V, and T for the neon. Use this to calculate the number of moles of neon which doesn't change when the new gas is added.]

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

Ammonia, NH3, may react with oxygen to form nitrogen gas and water. 4NH3(aq)+302(g)→2N2(g)+6H2O(1) If 3.45 g NH3 reacts with 5.18g 02 and produces 0.950L N2 at 295 K and 1.00 bar, how many moles of N2N2 can be produced by each reactant? It may be useful to consult the periodic table. mol N2 NH3: 02: mol N2 Based on the theoretical yields, which reactant is limiting? NH3(aq) O2(g) What is the percent yield of the reaction? percent yield:
A tire at a pressure of 760 kPa is heated from 0°C to 100.0°C. What is the new pressure?
Consider the following situation: You have a 50 L tank of compressed air at 15 atm and 100 ºC. You then pass the compressed air through a "titanium getter" which contains fragments of hot titanium metal. The purpose of the "getter" is to remove oxygen gas from the sample as Ti reacts with oxygen to form solid TiO2 (known as titania). Once the purified air is passed through the getter is it cooled back down to 100 ºC and fills another 50 L storage tank. If air typically contains about 20% oxygen, what could the pressure in the storage tank be? Question 2 options: A) 12 atm B) 15 atm C) 18 atm D) 24 atm
A gas sample has a mass of 1.211 g and occupies a volume of 677 mL. The temperature in the laboratory is 23 ⁰C and the gas pressure is 100. kPa. What is the molar mass of the gas?
I need help with part A and B
A small carbon dioxide gas cylinder used to propel paint balls has a mass of 56.3g. When all the gas is expelled from the cylinder and the cartridge is empty, the cylinder has a mass of 50.4g. If the volume of the cylinder is 25cm3 and the temperature of the cylinder was initially 23 c, determine the initial pressure of the gas.
Phosgene, COCl2, gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide and chlorine.CO(g)+Cl2(g)COCl2(g)The value of Kc for this reaction is 5.00 at 600 K.The reaction vessel initially contains a mixture of the reactants in which PCO = PCl2 = 0.2255 atm and PCOCl2 = 0 atm. What is the equilibrium partial pressure of CO? atm What is the equilibrium partial pressure of Cl2? atm What is the equilibrium partial pressure of COCl2? atm
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?
Calculate the temperature in oC for a 1.9 moles of carbon dioxide in a 1,290 mL container at a pressure of 495.2 kPa. Note: R = 0.08206 L atm/(K mol).
A 5.65 L vessel contains 22.0 g of PC13 and 3.35 g of O2 at 15.0 °C. The vessel is heated to 215 °C, and the contents react to give POC13. What is the final pressure in the vessel, assuming that the reaction goes to completion and that all reactants and products are in the gas phase? -- ΑΣΦ P= 1.441 ? atm