7 [Review Topics]Use the References to access important values if neededfor this question.How many grams of iron are needed tocompletely consume 49.5 L of chlorine gasaccording to the following reaction at 25 °C and1 atm?iron (s) + chlorine ( g ) – iron(III)chloride (s)gramsironDatni Entire Group

Given Volume of chlorine gas = 49.5 L Temperature = 25 oC Pressure = 1 atm

Answered: How many grams of iron are needed to…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter9: The Gaseous State

Section: Chapter Questions

Problem 70AP

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When ammonium nitrate decomposes at 722C, nitrogen, oxygen, and steam are produced. A 25.0-g sample of ammonium nitrate decomposes, and the products are collected at 125C into an evacuated flask with a volume of 15.0 L. (a) Write a balanced equation for the reaction. (b) What is the total pressure in the collecting flask after decomposition is complete?
Oxygen Consumption If 5.00 L of hydrogen gas,measured at a temperature of 20.0°C and a pressure of80.1 kPa, is burned in excess oxygen to form water, whatmass of oxygen will be consumed? Assume temperatureand pressure remain constant.
A 36.0—L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 350 g CO2, 805 g 02, and 4,880 g N2. At 25 degrees C. what is the pressure in the cylinder in atmospheres?
The chlorofluorocarbon CCl2F2 can be recycled into a different compound by reaction with hydrogen to produce CCl2F2(g), a compound useful in chemical manufacturing: CCl2F2(g)+4H2(g)CH2F2(g)+2HCl(g) (a) Outline the steps necessary to answer the following question: What volume of hydrogen at 225 atm and 35.5 C would be required to react with 1 ton (1.000103kg) of CCl2F2? (b) Answer the question.
95 Some engineering designs call for the use of compressed air for underground work. If water containing iron(II) ions is present, oxygen in the compressed air may react according to the following unbalanced net ionic equation: Fe2++H++O2Fe3++H2O (a) Write the balanced net ionic equation. Remember that the amounts of each substance and the charges must balance. (b) Assume all of the oxygen from 650 L of compressed air at 15°C and 6.5 atm is lost by this reaction. What mass of water would be produced? (The mole fraction of oxygen in air is about 0.21.) (c) What will be the final pressure after the loss of the oxygen?
Liquid oxygen was first prepared by heating potassium chlorate, KClO3, in a closed vessel to obtain oxygen at high pressure. The oxygen was cooled until it liquefied. 2KClO3(s)2KCl(s)+3O2(g) If 171 g of potassium chlorate reacts in a 2.70-L vessel, which was initially evacuated, what pressure of oxygen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.
Ammonium nitrate can be used as an effective explosive because it decomposes into a large number of gaseous products. At a sufficiently high temperature, ammonium nitrate decomposes into nitrogen, oxygen, and steam. (a) Write a balanced net ionic equation for the decomposition of ammonium nitrate. (b) If 2.00 kg of ammonium nitrate are sealed in a 50.0-L steel drum and heated to 745C, what is the resulting pressure in the drum after decomposition? (Assume 100% decomposition.)

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How many grams of iron are needed to completely consume 49.5 L of chlorine gas according to the following reaction at 25 °C and 1 atm? iron (s) + chlorine ( g ) – iron(III) chloride (s) grams iron