Concept explainers
(a)
Interpretation:
By burning sulfur with oxygen sulfur trioxide can be prepared:
A 5.00 L flask having 5 g of oxygen and sulfur at a temperature of 25 0C and pressure of 995 mm Hg is heated. The temperature in the flask increases to 138 0C after the completion of reaction. The pressure of SO3 in the flask needs to be calculated.
Concept introduction:
According to the
The molarity of the solution is calculated as follows:
Here, n is number of moles of solute and V is volume of solution in L.
Answer to Problem 91QAP
1.05 atm
Explanation of Solution
By burning sulfur with oxygen sulfur trioxide can be prepared
In the 5 g of sulfur the mole of sulfur present is:
Moles of sulfur reacted is 0.156 mol.
Similarly, number of moles of oxygen can be calculated using the ideal gas equation as follows:
The given pressure can be converted into atm as follows:
Thus,
The given temperature can be converted into Kelvin as follows:
Thus,
Putting the values,
From the balanced chemical reaction, 2 mol of S must react with 3 mol of
The number of moles of oxygen gas given is 0.268 mol thus, it is present in excess and the sulfur is limiting reactant.
The number of moles of SO3 produced is same as that of sulfur.
After completion of reaction, the volume is 5.00 L, temperature is 138 0C and the pressure in the flask due to SO3 is calculated as below:
Therefore, the pressure of SO3 is 1.05 atm.
(b)
Interpretation:
The total pressure in the flask needs to be determined.
Concept introduction:
The ideal gas equation is as follows:
Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.
Answer to Problem 91QAP
1.27 atm.
Explanation of Solution
The molar ratio of O2 :S is 3:2. The moles of oxygen used to react with 0.156 mol of sulfur are calculated as below:
Therefore, the moles of O2 used in 0.156 mol of sulfur are 0.234 mol.
The pressure in the flask prior the reaction is 995 mm Hg. The moles of O2 present initially a 25 0C are calculated as below:
Therefore, mole of oxygen present in the mixture is 0.268 mol.
The oxygen which is left unreacted is calculated as below:
The total number of moles in the flask =
The total number of moles in the flask is 0.190 mol.
The total pressure of gas in the flask due to SO3 and unreacted oxygen is calculated as
Therefore, the total pressure in the flask is 1.27 atm.
(c)
Interpretation:
The molarity of H2 SO4 formed if 250.0 mL is added into the flask needs to be determined.
Concept introduction:
According to the ideal
The molarity of the solution is calculated as follows:
Here, n is number of moles of solute and V is volume of solution in L.
Answer to Problem 91QAP
0.03 M.
Explanation of Solution
The volume of the flask containing SO3 is 5.00 L, if 250.0 mL of water is added, the total volume of solution becomes:
The molarity of solution is calculated as follows:
The moles of SO3 is 0.156 mol. The molarity of H2 SO4 is calculated as below:
Therefore, the molarity of H2 SO4 is 0.03 M.
Want to see more full solutions like this?
Chapter 5 Solutions
Chemistry: Principles and Reactions
- 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.arrow_forwardRaoul Pictet, the Swiss physicist who first liquefied oxygen, attempted to liquefy hydrogen. He heated potassium formate, KCHO2, with KOH in a closed 2.50-Lvessel. KCHO2(s)+KOH(s)K2CO3(s)+H2(g) If 75.0 g of potassium formate reacts in a 2.50-L vessel, which was initially evacuated, what pressure of hydrogen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.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
- 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?arrow_forwardYou have two pressure-proof steel cylinders of equal volume, one containing 1.0 kg of CO and the other containing 1.0 kg of acetylene, C2H2. (a) In which cylinder is the pressure greater at 25 C? (b) Which cylinder contains the greater number of molecules?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 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 mixture contained zinc sulfide, ZnS, and lead sulfide, PbS. A sample of the mixture weighing 6.12 g was reacted with an excess of hydrochloric acid. The reactions are ZnS(s)+2HCL(aq)ZnCl2(aq)+H2S(g)PbS(s)+2HCL(aq)PbCl2(aq)+H2S(g) If the sample reacted completely and produced 1.049 L of hydrogen sulfide, H2S, at 23C and 762 mmHg, what were the percentages of ZnS and PbS in the mixture?arrow_forwardYou have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?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_forwardA 1.0-L flask contains 10.0 g each of O2 and CO2 at 25 C. (a) Which gas has the greater partial pressure, O2 or CO2, or are they the same? (b) Which molecules have the greater rms speed, or are they the same? (c) Which molecules have the greater average kinetic energy, or are they the same?arrow_forwardIf the rms speed of He atoms in the exosphere (highest region of the atmosphere) is 3.53 103 m/s, what is the temperature (in kelvins)?arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning