(a)
Interpretation:
The reaction that produces most
Concept introduction:
Hydrogen is a minor component of atmosphere and very less in Earth’s crust also. It is one of the most important substances in
(b)
Interpretation:
The solid that produces most
Concept introduction:
Hydrogen is a minor component of atmosphere and very less in Earth’s crust also. It is one of the most important substances in Inorganic chemistry as it is used as the precursor of many compounds. Hydrogen gas is very good reducing agent as it is used in the reduction of different metal oxide to their respective metals by heating at high temperature. It is one of the components of water gas also. Hydrogen gas is mainly produced by the reaction of metal and metal hydrides with water.
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General Chemistry: Principles and Modern Applications - With Solutions Manual and Modified MasteringChemistry Code
- Consider a sealed container half-filled with water. Which statement best describes what occurs in the container? a. Water evaporates until the air is saturated with water vapor; at this point, no more water evaporates. b. Water evaporates until the air is overly saturated (super-por: at this point, no more water evaporates. Water evaporates until the air is overly saturated (supersaturated) with water, and most of this water recondenses; this cycle continues until a certain amount of water vapor is present, and then the cycle ceases. c. Water does not evaporate because the container is sealed. d. Water evaporates. and then water evaporates and recondenses simultaneously and continuously. e. Water evaporates until it is eventually all in vapor form. Explain each choice. Justify your choice, and for choices you did not pick. explain what is wrong with them.arrow_forwardWhen water is added to a mixture of aluminum metal and sodium hydroxide, hydrogen gas is produced. This is the reaction used in commercial drain cleaners: 2Al(s)+6H2O(l)+2OH(aq)2Al(OH)4(aq)+3H2(g)A sufficient amount of water is added to 49.92 g of NaOH to make 0.600 L of solution; 41.28 g of Al is added to this solution and hydrogen gas is formed. (a) Calculate the molarity of the initial NaOH solution. (b) How many moles of hydrogen were formed? (c) The hydrogen was collected over water at 25C and 758.6 mm Hg. The vapor pressure of water at this temperature is 23.8 mm Hg. What volume of hydrogen was generated?arrow_forwardMagnesium sulfate (MgSO4) has a solubility of 38.9 g/ 100 g H2O at 30C. A solution is prepared by adding 9.50 g of MgSO4 to 25.0 g of water at 40C. A homogeneous mixture is obtained. Is the solution saturated, unsaturated, or supersaturated? One gram of magnesium sulfate is added to the solution cooled to 30C. Would you expect some of the MgSO4 to precipitate? If so, how much? If not, how much more MgSO4 can be added before precipitation takes place?arrow_forward
- A solution is prepared by diluting 0.7850 L of 1.262 M potassium sulfide solution with water to a final volume of 2.000 L. (a) How many grams of potassium sulfide were dissolved to give the original solution? (b) What are the molarities of the potassium sulfide, potassium ions, and sulfide ions in the diluted solution?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_forwardHydrogen gas can be prepared by the reaction of zinc with hydrochloric acidas shown below:2 HCl (aq) + Zn (s) → ZnCl2 (aq) + H2 (g)Calculate the volume of hydrogen gas that is produced at 20.0 C and740. mm Hg from 2.750 g of zinc and an excess of hydrochloric acidarrow_forward
- Assume that 13.5g of solid aluminum react with excess HCl according to the following balanced equation at 19.0 °Cand 1.12atm: ???(?)+????(??)→??????(??)+???(?) a. How many moles of HCl are used in the reaction? b. What volume of hydrogen gas is produced?arrow_forward1. 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_forwardA 0.158-g sample of unknown metal, X, reacted with hydrochloric acid according to the following balanced reaction: 2 X (s) + 6HCl (aq) -> 2 XCl3 (aq) + 3 H2 (g) The volume of the hydrogen gas collected over water was 216 mL at 22 degress C and a barometer reading of 764 mm Hg (VP of water at 22 degrees C is 20. mm Hg) (a) Determine moles of "X" that would have been present initially to produce those moles of hydrogen using the mole ratio in the balanced equation above.arrow_forward
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