Concept explainers
Dinitrogen monoxide,
Write a balanced chemical equation for this reaction, treating all substances as gases. Include phases in your equation.
Two reservoirs, separated by a closed valve (of negligible volume), are filled with the reactants (one on each side). The pressure of
mg src=Images/HTML_99425-13-98QAP_image001.jpg alt="" align="top"/>
e valve between the reservoirs is opened, and the
What is the partial pressure of
(a)
Interpretation:
To write the balanced chemical equation between nitrogen monoxide and propane that results in the production of N2, CO2 and H2 O gases.
Concept Introduction:
According to Dalton’s atomic theory matter cannot be destroyed or created; in order to be consistent with this, one must make sure that the number of atoms for each distinct type of an element must be equal on both sides of a chemical reaction.
Answer to Problem 98QAP
The balanced chemical equation between nitrogen monoxide and propane that results in the production of N2, CO2 and H2 O gases is:
Explanation of Solution
Nitrogen monoxide and propane are the two reactants while N2, CO2 and H2 O are the products. The chemical equation with their phases is:
The above reaction is not balanced as the number of atoms of oxygen, carbon, and hydrogen is not same on both the sides of the reaction.
So, in order to balance the reaction, the
Thus, the balanced reaction is:
(b)
Interpretation:
The partial pressure of CO2 after the reaction undergoes completion should be determined.
Concept Introduction:
If there is a mixture of gasses in a container the total pressure exerted is the sum of partial pressure of the gasses present in the container. Partial pressure is defined as the pressure exerted by the gas if the gas was alone in the container.
Partial pressure can be derived as follows
Answer to Problem 98QAP
0.21 atm.
Explanation of Solution
The balanced chemical equation can be written as follows,
It is clearly specified in the question that all three main products are in gas state,
If
(c)
Interpretation:
The partial pressure of CO2 after the reaction undergoes completion should be calculated.
Concept Introduction:
If there is a mixture of gasses in a container the total pressure exerted is the sum of partial pressure of the gasses present in the container. Partial pressure is defined as the pressure exerted by the gas if the gas was alone in the container.
Partial pressure can be derived as follows
Answer to Problem 98QAP
Zero.
Explanation of Solution
Let partial pressure of
Hence it is clear that there is no
Want to see more full solutions like this?
Chapter 13 Solutions
Introductory Chemistry: A Foundation
- 109 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what volume of CO2 is evolved during the process. What would have to be measured to predict the needed volume in advance?arrow_forwardA sample of natural gas is 85.2% methane, CH4, and 14.8% ethane, C2H6, by mass. What is the density of this mixture at 18C and 771 mmHg?arrow_forwardA sample of a breathing mixture for divers contained 34.3% helium, He; 51.7% nitrogen, N2; and 14.0% oxygen, O2 (by mass). What is the density of this mixture at 22C and 775 mmHg?arrow_forward
- A chemist weighed out 5.14 g of a mixture containing unknown amounts of BaO(s) and CaO(s) and placed the sample in a 1.50-L flask containing CO2(g) at 30.0C and 750. torr. After the reaction to form BaCO3(s) and CaCO3(s) was completed, the pressure of CO2(g) remaining was 230. torr. Calculate the mass percentages of CaO(s) and BaO(s) in the mixture.arrow_forwardFor scuba dives below 150 ft, helium is often used to replace nitrogen in the scuba tank. If 15.2 g of He(g) and 30.6 g of O2(g) are added to a previously evacuated 5.00 L tank at 22 C, calculate the partial pressure of each gas present as well as the total pressure in the tank.arrow_forwardA mixture contained calcium carbonate, CaCO3, and magnesium carbonate, MgCO3. A sample of this mixture weighing 7.85 g was reacted with excess hydrochloric acid. The reactions are CaCO3(g)+2HCL(aq)CaCl2(aq)+H2O(I)+CO2(g)MgCO3(s)+2HCL(aq)MgCl2(aq)+H2O(I)+CO2(g) If the sample reacted completely and produced 1.94 L of carbon dioxide, CO2, at 25C and 785 mmHg, what were the percentages of CaCO3 and MgCO3 in the mixture?arrow_forward
- Earths atmosphere is approximately 80 N2 and 20 O2. If the total atmospheric pressure at sea level is about 14.7 lb/in2. where lb/in2 is pounds per square inch, a common but non-SI unit of pressure, what are the partial pressures of N2 and O2 in units lbs/in2?arrow_forward93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)arrow_forwardSulfur trioxide, SO3, is produced in enormous quantities each year for use in the synthesis of sulfuric acid. S(s)+O2(g)SO2(g)2SO2(g)+O2(g)2SO3(g) What volume of O2(g) at 350.C and a pressure of 5.25 atm is needed to completely convert 5.00 g sulfur to sulfur trioxide?arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning