Concept explainers
(a)
Interpretation : The partial pressure of hydrogen gas needs to be determined.
Concept Introduction : The ideal gas equation helps to calculate the pressure, volume, temperature of ideal gas as follows:
If a gas is collected over water, the total pressure always represents the sum of gas pressure and vapour pressure of water.
Hence;
Gas pressure = Total pressure - vapour pressure
(b)
Interpretation : The number of moles of hydrogen gas produced needs to be determined.
Concept Introduction : The ideal gas equation helps to calculate the pressure, volume, temperature of ideal gas as follows:
If a gas is collected over water, the total pressure always represents the sum of gas pressure and vapour pressure of water.
Hence;
Gas pressure = Total pressure - vapour pressure
Want to see the full answer?
Check out a sample textbook solutionChapter 11 Solutions
Basic Chemistry
- You 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_forwardIn the Mthode Champenoise, grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is C6H12O6(aq)2C2H5OH(aq)+2CO2(g) Fermentation of 750. mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total volume of 825 mL until 12% by volume is ethanol (C2H5OH). Assuming that the CO2 is insoluble in H2O (actually, a wrong assumption), what would be the pressure of CO2 inside the wine bottle at 25C? (The density of ethanol is 0.79 g/cm3.)arrow_forward5-111 Diving, particularly SCUBA (Self-Contained Underwater Breathing Apparatus) diving, subjects the body to increased pressure. Each 10. m (approximately 33 ft) of water exerts an additional pressure of 1 atm on the body. (a) What is the pressure on the body at a depth of 100. ft? (b) The partial pressure of nitrogen gas in air at 1 atm is 593 mm Hg. Assuming a SCUBA diver breathes compressed air, what is the partial pressure of nitrogen entering the lungs from a breathing tank at a depth of 100. ft? (c) The partial pressure of oxygen gas in the air at 2 atm is 158 mm Hg. What is the partial pressure of oxygen in the air in the lungs at a depth of 100. ft? (d) Why is it absolutely essential to exhale vigorously in a rapid ascent from a depth of 100. ft?arrow_forward
- When solid calcium carbonate is reacted with aqueous hydrochloric acid, the products of the reaction include aqueous calcium chloride, liquid water, and gaseous carbon dioxide. Calculate the volume of CO₂ gas (in L) collected over water at 25.0 °C when 25.1 g of calcium carbonate is added to excess hydrochloric acid if the total pressure is 911 mm Hg. The vapor pressure of water at 25.0 °C is 23.8 mm Hg.arrow_forwardThe temperature of your water was 22.4 degrees Celsius. The volume of hydrogen collected was 35.3 mL. The atmospheric pressure in the lab room was 29.60 inches Hg. The difference in the water level between the beaker and the burette is 20.0 cm. What was the mass of the magnesium ribbon used? Hint: 2 HCl(aq) + Mg(aq) = H2(g) + MgCl2(aq)arrow_forwardWhat volume of hydrogen gas (in mL) at 799 mm Hg and 26 °C can be produced when 2.8 g of MgCO3(s) are put into an Erlenmeyer flask containing 215 mL of 0.214 M HCl(aq) ?1 MgCO3(s) + 2 HCl(aq) → MgCl2(aq) + CO2(g) + H2O(l)arrow_forward
- 1. Where did the R constant in PV=nRT come from, and why must we convert everything to the units of the R constant? 2. Why does the density of water change with its temperature? 3. If all of the gas was not vaporized before taking the mass (some stayed in liquid form), how would that affect the final molar mass calculation? 4. If a sample of ethanol (C2H6O) was determined to have a pressure of 2 atm at a temperature of 25°C, what is its density (in g/L)?arrow_forwardWhen zinc metal is added to hydrochloric acid, the following reaction takes place Zn(s) + 2 HCI(aq) → ZnCl2(aq) + H2(g) Calculate the volume of H2 gas collected over water at 30.0 °C when 65.7 g of zinc is added to excess hydrochloric acid if the total pressure is 695 torr. The vapor pressure of water at 30.0 °C is 31.8 torr.arrow_forward8. For the reaction 2H₂O(1) + 2e¯ → H₂(g) + 2OH(aq), calculate the volume of "dry" hydrogen gas created at a pressure of 745 mm Hg and 25.0 °C when 0.6696 g H₂O are used. The vapor pressure of water at this temperature is 23.8 mmHg. A) 0.479 L B) 0.464 L C) 0.450 L D) 4.18 L E) 4.05 Larrow_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
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning