MISSED THIS? Read Section 6.6 (Pages 228-235); Watch KCV 6.6, IWE 6.10. A gas mixture contains 1.29 g N₂ and 0.76 g O₂ in a 1.64-L container at 15 °C. Y Part C Calculate the partial pressure of N₂. Express your answer using two significant figures. P₁ = Submit ▾ Part D P₁ = 195] ΑΣΦ Submit Request Answer Calculate the partial pressure of 0₂. Express your answer using two significant figures. 195] ΑΣΦ PAVIC ? Request Answer C atm atm

MISSED THIS? Read Section 6.6 (Pages 228-235); Watch KCV 6.6, IWE 6.10. A gas mixture contains 1.29 g N₂ and 0.76 g O₂ in a 1.64-L container at 15 °C. Y Part C Calculate the partial pressure of N₂. Express your answer using two significant figures. P₁ = Submit ▾ Part D P₁ = 195] ΑΣΦ Submit Request Answer Calculate the partial pressure of 0₂. Express your answer using two significant figures. 195] ΑΣΦ PAVIC ? Request Answer C atm atm

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter8: Gases

Section: Chapter Questions

Problem 155CP: Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/min at 1.50 atm and ambient...

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Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/min at 1.50 atm and ambient temperature. Air is added to the chamber at 1.00 atm and the same temperature, and the gases are ignited. a. To ensure complete combustion of CH4 to CO2(g) and H2O(g), three times as much oxygen as is necessary is reacted. Assuming air is 21 mole percent O2 and 79 mole percent N2, calculate the flow rate of air necessary to deliver the required amount of oxygen. b. Under the conditions in part a, combustion of methane was not complete as a mixture of CO2(g) and CO(g) was produced. It was determined that 95.0% of the carbon in the exhaust gas was present in CO2. The remainder was present as carbon in CO. Calculate the composition of the exhaust gas in terms of mole fraction of CO, CO2, O2, N2, and H2O. Assume CH4 is completely reacted and N2 is unreacted.
At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22C and a pressure of 734 torr. Calculate the mass percent of NaClO3 in the original sample. (At 22C the vapor pressure of water is 19.8 torr.)
A sample of potassium permaganate (KMnO4) reacts to completion with sodium oxalate (Na2C2O4) in the folowing redox reaction: 2MnO4- (aq) + 5C2O4-2 (aq) + 16H+ (aq) --> 10CO2 g) + 2Mn+2 (aq) + 8H2O (l) The volume of carbon dixoide released by the reaction at 297 K and 1.00 atm was 138 L. How many moles of potassium permanganate reacted? The Universal Gas Constant is 0.082057 L x atm/ mol x K. (answer in sig figs)
Combustible vapor-air mixtures are flammable over a limitedrange of concentrations. The minimum volume % of vapor thatgives a combustible mixture is called the lower flammable limit(LFL). Generally, the LFL is about half the stoichiometric mix-ture, the concentration required for complete combustion of thevapor in air. (a) If oxygen is 20.9 vol % of air, estimate the LFL forn-hexane, C₆H₁₄. (b) What volume (in mL) of n-hexane (d=0.660 g/cm³) is required to produce a flammable mixture of hexane in 1.000 m³of air at STP?
Nickel carbonyl, Ni(CO)4, is one of the most toxic substancesknown. The present maximum allowable concentrationin laboratory air during an 8-hr workday is 1 ppb(parts per billion) by volume, which means that there isone mole of Ni(CO)4 for every 109 moles of gas. Assume24 °C and 1.00 atm pressure. What mass of Ni(CO)4 is allowablein a laboratory room that is 12 ft x 20 ft x 9 ft?
sodium azide (Na3N) decomposes on heating to form sodium and nitrogen gas. 2Na3N--> 6Na+N2 1.35g of sodium nitride were heated. a) calculate the mass of sodium formed on complete decomposition of the sodium nitride. give your answer to 3 significant figures.(AO2) b)calculate the volume of nitrogen gas (in cm^3)produced on complete decomposition of 1.35g of sodium nitride at 320K and 110kpa. the gas constant R= 8.31JK^-1 mol^-1. give your answer to 3 significant figures. (AO2)
The thermal decomposition of potassium chlorate can be used to produce oxygen. 2KClO3 --> 2KCl +3O2 What volume of O2 gas at 298 K and 1.0 atm pressure is produced by the decomposition of 7.50 g of KClO3 (FW=122.6)?
14. At 373 K at 110 kPa, it was found that 1.00 L of gas ( assume ideal gas) weighed 2.95 g. Its molecular mass is?
(a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City (MCI) to Baltimore (BWI) burned 11,800 lb (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of CnH2n+2 hydrocarbons, with n =6 to 16, so the carbon:hydrogen ratio is close to 1:2. During this flight, how much CO2 was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO2 and H2O. Give both the mass of CO2 produced (in kg and in lbs) and the volume it would occupy at 298 K, 1 atm.(b) How much CO2 would be released into the atmosphere if those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg L-1 and that carbon and hydrogen dominate the composition in a ratio of 1:2. The road trip is 1082 miles.
1) Commercial fuming Sulphuric acid (Oleum-H2S2O6) is 99.9% solution. Please convert it into molarity.2) Find out the Volume (dm3) of product (gas) at RTP when 0.58 M, 150 mL NaOH (aq.) reacts with 350 mL, 0.25 NH4Cl.
Provided that a methane gas combust a 25 g, find the volume of O required under 298K and 0.21 atm?
A student performed the experiment described in this module, using 4.00 mL of a 3.5% H2O2 solution with a density of 1.61 g mL-1. The water temperature was 25 ° C, and the barometric pressure in the laboratory was 30.40 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 79.20 mL of O2. (8) Calculate the number of moles of H2O2 reacting.