Concept explainers
(a)
Interpretation:
The formula for the unknown gas and the balanced reaction has to be written.
Concept Introduction:
Balancing equations:
In a reaction, the number of molecules before and after the reaction should be equal. That means the number of moles of particular compound on either side of the reaction should be equal, this can be done by multiplication with the number of molecules required to make them equal in a reaction.
(b)
Interpretation:
The type formula has to be identified.
Concept Introduction:
Empirical formula:
The formula giving the quantities of the elements present in a compound but not the definite numbers or arrangement of atoms.
Molecular formula:
The number of atoms of every element present in a compound.
(c)
Interpretation:
The two possible electronic dot structures for
Concept Introduction:
Electron-dot structure:
The valence electrons are symbolized by dots placed around the chemical symbol. Electrons are positioned up to two on each side of the elemental symbol for a maximum of eight which is the number of electrons in a filled s and p shell.
(d)
Interpretation:
The
Concept Introduction:
Molar mass:
It is a physical property, which is defined as the mass of a given substance divided by the amount of substance. Unit of the kilogram is
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
General Chemistry: Atoms First
- Silane, SiH4, is the silicon analogue of methane, CH4. It is prepared industrially according to the following equations: Si(s)+3HC1(g)HSiCl3(l)+H2(g)4HSiCl3(l)SiH4(g)+3SiCl4(l) a. If 156 mL HSiCl3 (d = 1.34 g/mL) is isolated when 15.0 L HC1 at 10.0 atm and 35C is used, what is the percent yield of HSiCl3? b. When 156 mL HSiCl3 is heated, what volume of SiH4 at 10.0 atm and 35C will be obtained if the percent yield of the reaction is 93.1%?arrow_forwardTitanium(III) chloride is used in the manufacture of polyethylene. It is produced by the reaction (at high temperatures) between TiCl4 gas and H2. 2TiCl4(g)+H2(g)2TiCl3(s)+2HCl(g)Assume 100% yield and constant temperature and pressure. (a) How many liters of HCI gas can be produced by mixing 3.72 L of TiCl4 and 4.50 L of H2? (b) How many liters of reactant in excess are present after the reaction is complete?arrow_forward5-114 Carbon dioxide gas, saturated with water vapor, can be produced by the addition of aqueous acid to calcium carbonate based on the following balanced net ionic equation: (a) How many moles of wet CO (g), collected at 60.°C and 774 torr total pressure, are produced by the complete reaction of 10.0 g of CaCO3 with excess acid? (b) What volume does this wet CO2 occupy? (c) What volume would the CO2 occupy at 774 torr if a desiccant (a chemical drying agent) were added to remove the water? The vapor pressure of water at 60.°C is 149.4 mm Hg.arrow_forward
- A 275-mL sample of CO gas is collected over water at 31C and 755 mmHg. If the temperature of the gas collection apparatus rises to 39C, what is the new volume of the sample? Assume that the barometric pressure does not change.arrow_forward61 As one step in its purification, nickel metal reacts with carbon monoxide to form a compound called nickel tetracarbonyl, Ni(CO)4, which is a gas at temperature above about 316 K. A 2.000-L flask is filled with CO gas to a pressure of 748 torr at 350.0 K, and then 5.00 g of Ni is added. If the reaction describe occurs and goes to completion at constant temperature, what will the final pressure in the falsk be?arrow_forward47 HCl(g) reacts with ammonia gas, NH3(g), to form solid ammonium chloride. If a sample of ammonia occupying 250 mL at 21 C and a pressure of 140 torr is allowed to react with excess HCl, what mass of NH4Cl will form?arrow_forward
- 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_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_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_forward
- 57 What volume of hydrogen gas, in liters, is produced by the reaction of 3.43 g of iron metal with 40.0 mL of 2.43 M HCl? The gas is collected at 2.25 atm of pressure and 23 C. The other product is FeCl2?arrow_forwardHydrogen gas is used in weather balloon because it is less expensive than Helium. Assume that 5.57 g of H2 is used to fill a weather balloon to an initial volume of 67 L at 1.04 atm. If the ballloon rises to an altitude where the pressure is 0.047 atm, what is its new volume? Assume that the temperature remains constant.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_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher: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
- 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