Assume that an exhaled breath of air consists of 74.6 % No. 15.5 % O2, 3.6 % CO2, and 6.3 % water vapor. Correct Part E Previous Answers If the volume of the exhaled gas is 460 mL, and its temperature is 37 °C calculate the number of moles of CO, exhaled.. Express your answer using two significant figures. Ο ΑΣΦ CO Submit Previous Answers Request Answer mol

Assume that an exhaled breath of air consists of 74.6 % No. 15.5 % O2, 3.6 % CO2, and 6.3 % water vapor. Correct Part E Previous Answers If the volume of the exhaled gas is 460 mL, and its temperature is 37 °C calculate the number of moles of CO, exhaled.. Express your answer using two significant figures. Ο ΑΣΦ CO Submit Previous Answers Request Answer mol

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter10: Gases And Their Properties

Section: Chapter Questions

Problem 105IL: You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find...

See similar textbooks

Similar questions

You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.
62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?
Pyruvic acid, HC3H3O3, is involved in cell metabolism. It can be assayed for (that is, the amount of it determined) by using a yeast enzyme. The enzyme makes the following reaction go to completion: HC3H3O3(aq)C2H4O(aq)+CO2(g) If a sample containing pyruvic acid gives 21.2 mL of carbon dioxide gas, CO2, at 349 mmHg and 30C, how many grams of pyruvic acid are there in the sample?
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?
A student prepares phosphorous acid, H3PO3, by reacting solid phosphorus triiodide with water. PI3(s)+3H2O(l)H3PO3(s)+3HI(g) The student needs to obtain 0.250 L of H3PO3(d=1.651g/cm3). The procedure calls for a 45.0% excess of water and a yield of 75.0%. How much phosphorus triiodide should be weighed out? What volume of water (d=1.651g/cm3) should be used?
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?
On combustion, 1.0 L of a gaseous compound of hydrogen, carbon, and nitrogen gives 2.0 L of CO2, 3.5 L of H2O vapor, and 0.50 L of N2 at STP. What is the empirical formula of the compound?