How many moles of an ideal gas are there at a pressure of 854 torr, a volume of 5.2 L, and a temperature of 273K?Answer:

Following ideal gas equation: PV = nRT In this question, either convert unit of pressure from torr…

Answered: How many moles of an ideal gas are…

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU3: Weather: Phase Changes And Behaviour Of Gases

Section: Chapter Questions

Problem 19STP

See similar textbooks

Similar questions

What is the density of laughing gas, dinitrogen monoxide, N2O, at a temperature of 325 K and a pressure of 113.0 kPa?
5-54 Automobile air bags are inflated by nitrogen gas. When a significant collision occurs, an electronic sensor triggers the decomposition of sodium azide to form nitrogen gas and sodium metal. The nitrogen gas then inflates nylon bags, which protect the driver and front-seat passenger from impact with the dashboard and windshield. What volume of nitrogen gas measured at 1 atm and 27°C is formed by the decomposition of 100. g of sodium azide?
5.27 A newly discovered gas has a density of 2.39 g/L at 23.0°C and 715 mm Hg. What is the molar mass of the gas?
A 0.245-L flask contains 0.467 mol CO2 at 159 C. Calculate the pressure: (a) using the ideal gas law (b) using the van der Waals equation (c) Explain the reason for the difference. (d) Identify which correction (that for P or V) is dominant and why.
41 A sample of a smokestack emission was collected into 1.25-L tank at Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass. What is the partial pressure exerted by gas?
Before small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas. C2H2, and solid calcium hydroxide were formed by the reaction of calcium carbide, CaC2. with water. The ignition of the acetylene gas provided the light. Currently, the same lamps are used by some cavers, and calcium carbide is used to produce acetylene for carbide cannons. (a) Outline the steps necessary to answer the following question: What volume of C2H2 at 1.005 atm and 12.2 C is formed by the reaction of 15.48 g of CaC2 with water? (b) Answer the question.
A mixture of N2 and Ne contains equal moles of each gas and has a total mass of 10.0 g. What is the density of this gas mixture at 500 K and 15.00 atm? Assume ideal gas behavior.
60 Automakers are always investigating reactions for the generation of gas to inflate air bags, in part the because the sodium produced in the decomposition of NaN3 (see Problem 5.59) presents safety concerns. One system that has been considering is the oxidation of graphite by Strontium nitrate, as Sr(NO3)2as shown in the equation below: 5C(s)+2Sr(NO3)2(s)2SrO(s)+2N2(g)+5CO2(g) . Suppose that a System is being designed using this reaction and the goal is to generate enough gas to inflate a bag 61 L and 1.3 atm at 23 C. What is the minimum mass of graphite that should be used in the design of this system?
55 Ammonia is not the only possible fertilizer. Others include urea, which can be produced by the reaction: CO2(g)+2NH3(g)CO(NH2)2(s)+H2O(g) A scientist has 75 g of dry ice to provide the carbon dioxide. If 4.50 L of ammonia at 15 C and a pressure of 1.4 atm is added, which reactant is limiting? What mass of urea will form?
48 Hydrogen gas is generated when acids come into contact with certain metals. When excess hydrochloric acid reacts with 2.5 g of Zn (the metal product is Zn2+), what volume of hydrogen gas is collected at a pressure of 0.93 atm and a temperature of 22 C?
What is the value of the ideal gas constant R if the volume is specified in milliliters rather than liters?
Calculate the molar volume of ethane at 1.00 atm and 0C and at 10.0 atm and 0C, using the van der Waals equation. The van der Waals constants are given in Table 5.7. To simplify, note that the term n2a/V2 is small compared with P. Hence, it may be approximated with negligible error by substituting nRT/P from the ideal gas law for V in this term. Then the van der Waals equation can be solved for the volume. Compare the results with the values predicted by the ideal gas law.

SEE MORE QUESTIONS

Recommended textbooks for you

Living by Chemistry

Chemistry

ISBN:

9781464142314

Author:

Angelica M. Stacy

Publisher:

W. H. Freeman

General, Organic, and Biological Chemistry

Chemistry

ISBN:

9781285853918

Author:

H. Stephen Stoker

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Living by Chemistry

Chemistry

ISBN:

9781464142314

Author:

Angelica M. Stacy

Publisher:

W. H. Freeman

General, Organic, and Biological Chemistry

Chemistry

ISBN:

9781285853918

Author:

H. Stephen Stoker

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

SEE MORE TEXTBOOKS

How many moles of an ideal gas are there at a pressure of 854 torr, a volume of 5.2 L, and a temperature of 273 K? Answer: