Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makeseasy to isolate and measure the amount of gas produced.collectedgasSuppose the C0 gas evolved by a certain chemical reaction taking place at 50.0 °C is collected over water, using anapparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be28.6 mL.chemicalreactionwaterSketch of a gas-collection apparatusCalculate the mass of CO that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption aboutthe reaction conditions and the nature of the gases.ExplanationCheckO 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy CenterAccessibilitydtv2444DII19**S0F6FSF4escF3F22$delete6.7934.52PYQWR...* 00

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Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. collected gas chemical reaction water Suppose the C0 gas evolved by a certain chemical reaction taking place at 50.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 28.6 mL. Sketch of a gas-collection apparatus Calculate the mass of CO that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases.

Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. collected gas chemical reaction water Suppose the C0 gas evolved by a certain chemical reaction taking place at 50.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 28.6 mL. Sketch of a gas-collection apparatus Calculate the mass of CO that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about the reaction conditions and the nature of the gases.

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

Chapter5: Gases

Section: Chapter Questions

Problem 35Q

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes
easy to isolate and measure the amount of gas produced.
collected
gas
Suppose the C0 gas evolved by a certain chemical reaction taking place at 50.0 °C is collected over water, using an
apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be
28.6 mL.
chemical
reaction
water
Sketch of a gas-collection apparatus
Calculate the mass of CO that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about
the reaction conditions and the nature of the gases.
Explanation
Check
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Accessibility
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93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
You have a 550.-mL tank of gas with a pressure of 1.56 atm at 24 C. You thought the gas was pure carbon monoxide gas, CO, but you later found it was contaminated by small quantities of gaseous CO2 and O2. Analysis shows that the tank pressure is 1.34 atm (at 24 C) if the CO2 is removed. Another experiment shows that 0.0870 g of O2 can be removed chemically. What are the masses of CO and CO2 in the tank, and what is the partial pressure of each of the three gases at 25 C?
Many nitrate salts can be decomposed by heating. For example, blue, anhydrous copper(II) nitrate produces the gases nitrogen dioxide and oxygen when heated. In the laboratory, you find that a sample of this salt produced a 0.195-g mixture of gaseous NO2 and O2 with a total pressure of 725 mm Hg at 35 C in a 125-mL flask (and black, solid CuO was left as a residue). What is the average molar mass of the gas mixture? What are the mole fractions of NO2 and O2 in the mixture? What amount of each gas b in the mixture? Do these amounts reflect the relative amounts of NO2 and O2 expected based on the balanced equation? Is it possible that the fact that some NO2 molecules combine to give N2O4 plays a role? Heating copper(II) nitrate produces nitrogen dioxide and oxygen gas and leaves a residue of copper(ll) oxide.
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105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so unusual the process was once used in fireworks displays. There are actually several reactions that take place when the solid Hg(SCN)2 is ignited: 2Hg(SCN)2(s)2HgS(s)+CS2(s)+C3N4(s)CS2(s)+3O2(g)CO2(g)+2SO2(g)2C3N4(s)3(CN)2(g)+N2(g)HgS(s)+O2(g)Hg(l)+SO2(g) A 42.4-g sample of Hg(SCN)2 is placed into a 2.4-L vessel at 21°C. The vessel also contains air at a pressure of 758 torr. The container is sealed and the mixture is ignited, causing the reaction sequence above to occur. Once the reaction is complete, the container is cooled back to the original temperature of 21°C. (a) Without doing numerical calculations, predict whether the final pressure in the vessel will be greater than, less than, or equal to the initial pressure. Explain your answer. (b) Calculate the final pressure and compare your result with your prediction. (Assume that the mole fraction of O2 in air is 0.21.)
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perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
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5-56 The three main components of dry air and the percentage of each are nitrogen (78.08%), oxygen (20.95%), and argon (0.93%). (a) Calculate the partial pressure of each gas in a sample of dry air at 760 mm Hg. (b) Calculate the total pressure exerted by these three gases combined.
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