Concept explainers
Interpretation:
The total volume and the partial pressures of the gases formed from the decomposition of nitroglycerin are to be calculated.
Concept Introduction:
The expression foran ideal gas equation is
Here,
The expression to calculate mole fraction
Here,
The relation between partial pressure
The number of moles is given by the expression, which is as:
The conversion factor is
So the moles can be calculated by the expression as:
The conversion of temperature from degree Celsius to Kelvin can be done by using the formula given below:
Answer to Problem 98AP
Solution:
Explanation of Solution
Given information:
Pressure is
Mass of nitroglycerine is
The mass of
Invert the conversion factor, whichbecomes
According to the given reaction, the mole ratio of nitroglycerine and the products is
Therefore, the conversion factor becomes
Multiply the conversion factors with the mass of nitroglycerine in order to calculate the moles of the products as
The moles can be calculated by the expression as
Temperature is in Celsius. Convert it into Kelvin as:
The expression foran ideal gas equation is
Rearrange the above expression for
Substitute
As the minimum number of significant figures is 2, the final answer should also contain two significant figures, that is,
The relation between partial pressure and total pressure is
The formula to calculate the mole fraction is
Now, calculate the mole fractions of each product.
For
For
For
For
For
For
For
For
The total volume of the gas is
Want to see more full solutions like this?
Chapter 10 Solutions
Chemistry
- A 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_forwardGiven that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?arrow_forwardA 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_forward
- 0.17 moles of hydrogen gas and 0.33 moles of nitrogen gas are created from thereaction 2NH3 (g) → 3H2 (g) + N2 (g). The final total pressure in the reaction vessel is0.75 atm. Calculate the partial pressure of the hydrogen gas at the end of the reaction.Assume the number of moles of NH3 (g), left after the reaction occurs, is negligible.arrow_forwardYou are trying to determine, by experiment, the formula of a gaseous hydrofluorocarbon compound you made to replace chlorofluorocarbons in air conditioners. You have determined the empirical formula is CHF₂, but now you want to know the molecular formula. You therefore do an experiment to determine its molar mass and find that a 0.100-g sample of the compound exerts a pressure of 69.0 mm Hg in a 263-mL container at 23.1 °C. What is the molar mass of the compound? What is its molecular formula? Enter the elements of the formula in the order C, H, F. g/mol Molecular formula =arrow_forwardConsider a rigid 21.44 L gas canister that holds a mixture of two gases, Cl₂ and Xe. The total number of moles in the container is 6.71 moles, and the container is held at 25 degrees Celsius. If there are 1.77 moles of Xe in the container, what is the partial pressure of Cl₂ in the gas mixture? Express your answer in terms of atm using at least three significant figures.arrow_forward
- The volume of a sample of pure HCI gas was 239 mL at 24°C and 177 mmHg. It was completely dissolved in about 70 mL of water and titrated with an NaOH solution; 28.5 mL of the NaOH solution was required to neutralize the HCI. Calculate the molarity of the NaOH solution. Marrow_forwardConsider the generic reaction: A (g) → 2 B (g) + C (g) . If a flask initially contains only A and the reaction proceeds to completion with a final pressure of 49.8 atm , what is the partial pressure of B in the container? (Assume constant volume and temperature.) Express your answer numerically and in terms of atm.arrow_forwardYou are given 2.263 g of a mixture of KClO3 and KCl. When heated, the KClO3 decomposes to KCl and O2, 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g), and 632 mL of O2 is collected over water at 20 °C. The total pressure of the gases in the collection flask is 736 mm Hg. What is the weight percentage of KClO3 in the sample? The formula weight of KClO3 is 122.55 g/mol. The vapor pressure of water at 20 °C is 17.5 mm Hg.arrow_forward
- A sample of 263.0 mL of wet nitrogen gas was collected over water at a total pressure of 756 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH,SO3, with 368.5 mL of a solution of sodium nitrite according to the following equation. NaNO2 + HNH2SO3- N2 + NaHSO4 + H2O Calculate what must have been the molar concentration of the sodium nitrite. Marrow_forwardZinc reacts with hydrochloric acid to produce hydrogen gas (as shown by the following equation). If 47.4 mL of gas is collected over water at 30°C and with an atmospheric pressure of 766.3 mmHg, how much hydrochloric acid was consumed? Give your answer in millimoles (mmol) to 3 sig figs. Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq)arrow_forwardA sample of hydrogen gas was collected by displacement of water in a large gas buret. The total pressure in the buret was measured as 764.2 torr, the temperature was 23.0 °C, and the buret contained 511 mL of the collected gas. How many moles of hydrogen were collected? (At 23.0 °C, the vapor pressure of water is 21.1 torr.)arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher: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