Concept explainers
A concentration of 8.00 × 102 ppm by volume of CO is considered lethal to humans. Calculate the minimum mass of CO in grams that would become a lethal concentration in a closed room 17.6 m long, 8.80 m wide, and 2.64 m high. The temperature and pressure are 20.0°C and 756 mmHg, respectively.
Interpretation:
The minimum mass of carbon monoxide would become poisonous to humans in a closed room has to be calculated.
Concept Introduction:
Partial pressure:
The product of total pressure of gases and number of mole of individual gas is the partial pressure of a gas.
Mole fraction:
Mole fraction is the ratio number of moles of a species to that of total number of moles of solution.
Ideal gas equation:
The ideal gas equation is given as
Where,
P is the pressure
V is the volume
n is number of moles
R is the gas constant
T is the temperature
The volume of the closed room is calculated as,
Answer to Problem 20.65QP
The minimum mass of carbon monoxide would become poisonous to humans in a closed room is
Explanation of Solution
Given,
Temperature
Total pressure
Length of the closed room
Wide of the closed room
Height of the closed room
The volume of the closed room is calculated as,
The mole fraction of
From the total pressure and mole fraction of carbon monoxide, the partial pressure is calculated as,
The number of moles of carbon monoxide is calculated as,
The mass of carbon monoxide is calculated using molar mass of carbon monoxide as,
Want to see more full solutions like this?
Chapter 20 Solutions
AVC LOOSELEAF CHEMISTRY W/CONNECT 2 SEM
- When calcium carbonate is heated strongly, it evolves carbon dioxide gas. CaCO3(s)CaO(s)+CO2(g) 25 g of CaCO3 is heated, what mass of CO2would be produced? What volume would this quantity of CO2 (CU at STP?arrow_forwardSuppose you are performing a gas-producing reaction to experimentally determine the molar volume of the gas. Mg (s) + 2 HC1 (aq) → MgCl₂ (aq) + H₂ (g) A sample of Mg produces 21.5 mL of H₂ gas. The gas is collected over water at an atmospheric pressure of 769.6 mm Hg at 22 °C, at which the vapor pressure of water is 19.8 mm Hg. What is the experimental value for the molar volume of the hydrogen gas in L/mol?arrow_forwardIn Module #4, we discussed the role of chlorofluorocarbons (CFCs) in catalyzing the destruction of O3 in the stratosphere. One example of a CFC that is known to exasperate formation of the hole in the O3 layer is dichlorodifluoromethane (CF2Cl2). In the year 2000, this chemical reached its peak concentration of 2.2 x 10-11 M in the atmosphere. The destruction of CF2Cl2 can be approximated as a first-order process and the 1996 treaty on CFC emissions has eliminated its release into the atmosphere. Given that the rate constant for destruction of CF2Cl2 in the atmosphere is 0.009 yr-1, how long will it take for the concentration of CF2Cl2 to decline to 0.22 x 10-11 M?arrow_forward
- Potassium chlorate, potassium chloride, and water is produced by passing chlorine gas into a hot solution of potassium hydroxide. Calculate the volume in L of chlorine gas needed to produce 724.25 mL of 4.25 M potassium chlorate. The density of chlorine gas is 3.17 g/L. Atomic Mass: K: 39.098 g/mol Cl: 35.453 g/mol O: 15.999 g/mol H: 1.008 g/molarrow_forwardA student decides to conduct an experiment by using two different flasks and two different gas samples. In flask 1, there exists Neon (Ne) gas, whereas the second flask is filled with nitrogen (N2) gas. If both flasks are kept at 1 K, answer the following questions. (Note: Molar mass of N2 = 28.014 g mol1, molar mass of Neon = 20.1797 g mol1, R=8.31 J. mol.K-1, k= 1.38 x 10-23 J.K-1, Avogadro's number = 6.02 x 1023 mo/-1 :) a) Find the average kinetic energy of one Neon molecule. 6.21e-21 b) Calculate the average kinetic energy (translational+rotational) of one nitrogen molecule by including rotational motion in your calculations. 1.035e-20 J c) Find the root-mean-square speed of one neon molecule. 35.14 VV ms-1arrow_forwardPotassium chlorate, potassium chloride, and water is produced by passing chlorine gas into a hot solution of potassium hydroxide. Calculate the volume in L of chlorine gas needed to produce 604.17 mL of 4.64 M potassium chlorate. The density of chlorine gas is 3.17 g/L. Atomic Mass: K: 39.098 g/mol Cl: 35.453 g/mol O: 15.999 g/mol H: 1.008 g/mol Round your answer to 2 decimal places.arrow_forward
- The concentration of gold in seawater is 0.0027 ug/L. What mass of gold (in kg) is present in the Atlantic Ocean, of volume 3.23 x 1011 km3 ?arrow_forwardThe equation for photosynthesis is 6H2O (water) + 6CO2 (carbon dioxide) + Light Energy → C6H12O6 (glucose) + 6O2(oxygen). When first discovered, scientists were trying to decide if the oxygen in the product came from carbon dioxide or water. Which statement describes how scientists traced the path of oxygen?arrow_forwardThe allowable concentration level of vinyl chloride, C2H3Cl,in the atmosphere in a chemical plant is 2.0 x 10-6 g/L.How many moles of vinyl chloride in each liter does this represent?How many molecules per liter?arrow_forward
- A 4.80 mol4.80 mol sample of solid AA was placed in a sealed 1.00 L container and allowed to decompose into gaseous BB and C.C. The concentration of BB steadily increased until it reached 1.10 M,1.10 M, where it remained constant. A(s)−⇀↽−B(g)+C(g)A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of AA remain?arrow_forwardA concentration of carbon monoxide of 4000 ppm (0.400 % by mass) in air is lethal in about half an hour. What mass in grams of carbon monoxide in a car with an internal volume of 2.9 m3 is sufficient to provide that concentration? Assume the density of air is 1.29 g/L ; 1m3=1000L.arrow_forwardConsider the reaction 2 NO(g) + 5 H2(g) → 2 NH3(g) + 2 H20(g) The reaction mixture initially contains 6 moles of NO and 10 moles of H2 contained in a 20.0- liter gas cylinder with a movable piston. At the end of the reaction, the volume has decreased to 15.7 L. Without doing any calculations, which method is the best for determining the concentration of NO in the mixture after the reactants have reacted as completely as possible? Use stoichiometry: 10 moles of H2 consumes 6 moles of NO, so the final concentration of NO = 0 M Use the dilution formula: (6 mol NO)(20.0 L) = (x mol NO)(15.7 L) Use the dilution formula: (2 mol NO)(20.0 L) = (x mol NO)(15.7 L) Use stoichiometry: 10 moles of H2 consumes 4 moles of NO, so the final concentration of NO = (6 moles - 4 moles NO)/(15.7 L)arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning