4) Formaldehyde (CH2O) is a gas that can react in the following reaction: 3 CH2O(g) + 3 H2S(g) → (CH2S)3 (s) + 3 H2O(g) a) At STP, how many L of formaldehyde would be used if 7.88 g of the organic solid trithiane (MW= 138.3 g/mol) was produced? [ Select] b) At STP, how many L of water would be produced if 2.50 L of formaldehyde was reacted? [ Select ] c) what if part b) was done at 15C and 0.896 atm how many L of formaldehyde would be used? [ Select]

4) Formaldehyde (CH2O) is a gas that can react in the following reaction: 3 CH2O(g) + 3 H2S(g) → (CH2S)3 (s) + 3 H2O(g) a) At STP, how many L of formaldehyde would be used if 7.88 g of the organic solid trithiane (MW= 138.3 g/mol) was produced? [ Select] b) At STP, how many L of water would be produced if 2.50 L of formaldehyde was reacted? [ Select ] c) what if part b) was done at 15C and 0.896 atm how many L of formaldehyde would be used? [ Select]

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 111E

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Methanol (CH3OH) can be produced by the following reaction: CO(g)+2H2(g)CH3OH(g) Hydrogen at STP flows into a reactor at a rate of 16.0 L/min. Carbon monoxide at STP flows into the reactor at a rate of 25.0 L/min. If 5.30 g methanol is produced per minute, what is the percent yield of the reaction?
94 Mining engineers often have to deal with gases when planning for the excavation of coal. Some of these gases, including methane, can be captured and used as fuel to support the mining operation. For a particular mine, 2.4 g of CH4 is present for every 100.0 g of coal that is extracted. If 45.6% of the methane can be captured and the daily production of the mine is 580 metric tons of coal, how many moles of methane could be obtained per day?
Consider the following sketch. Each square in bulb A represents a mole of atoms X. Each circle in bulb B represents a mole of atoms Y. The bulbs have the same volume, and the temperature is kept constant. When the valve is opened, atoms of X react with atoms of Y according to the following equation: 2X(g)+Y(g)X2Y(g)The gaseous product is represented as and each represents one mole of product. (a) IfP A=2.0 atm, what is P8 before the valve is opened and the reaction is allowed to occur? What is P A+P B? (b) Redraw the sketch to represent what happens after the valve is opened. (c) What is PA? What is PB? What is P A+P B? Compare your answer with the answer in part (a).
84 Consider a sample of an ideal gas with n and T held constant. Which of the graphs below represents the proper relationship between P and V? How would the graph differ for a sample with a larger number of moles?
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.
A person exhales about 5.8 102 L of carbon dioxide per day (at STP). The carbon dioxide exhaled by an astronaut is absorbed from the air of a space capsule by reaction with lithium hydroxide, LiOH. 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) How many grams of lithium hydroxide are required per astronaut per day?
A flask is first evacuated so that it contains no gas at all. Then, 2.2 g of CO2 is introduced into the flask. On warming to 22 C, the gas exerts a pressure of 318 mm Hg. What is the volume of the flask?
Butyl mercaptan, C4H9SH, has a very bad odor and is among the compounds added to natural gas to help detect a leak of otherwise odorless natural gas. In an experiment, you burn 95.0 mg of C4H9SH and collect the product gases (SO2, CO2, and H2O) in a 5.25-L flask at 25 C. What is the total gas pressure in the flask, and what is the partial pressure of each of the product gases?
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?
61 As one step in its purification, nickel metal reacts with carbon monoxide to form a compound called nickel tetracarbonyl, Ni(CO)4, which is a gas at temperature above about 316 K. A 2.000-L flask is filled with CO gas to a pressure of 748 torr at 350.0 K, and then 5.00 g of Ni is added. If the reaction describe occurs and goes to completion at constant temperature, what will the final pressure in the falsk be?
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?
5-118 Isooctane, which has a chemical formula C8H18 is the component of gasoline from which the term octane rating derives. (a) Write the balanced chemical equation for the combustion of isooctane. (b) The density of isooctane is 0.792 g/mL. How many kg of C02 are produced each year by the annual U.S. gasoline consumption of L? (c) What is the volume in liters of this CO2 at STP? (d) The chemical formula for isooctane can be represented by (CH3)3CCH2CH(CH3)2. Draw a Lewis structure of isooctane. (e) Another molecule with the same molecular formula is octane, which can be represented by: When comparing isooctane and octane, one structure is observed to have a boiling point of 99°C, while another is known to have a boiling point Of 125°C. Which substance, isooctane or octane, is expected to have the higher boiling point? (f) Determine whether isooctane or octane is expected to have the greater vapor pressure.

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